[1/8/2002 2:26:24 PM | Mr. Fasciano]
1/8/2002 1:34:27 PM | Mr. Fasciano]
1) The study of the composition and structure of matter is the domain of which field of science?
A) biology B) geology C) physics D) chemistry
2) Which of the following changes would be most appropriately considered in a study of chemistry, rather than any other science?
A) a rock melting as the result of being heated
B) a rock rolling down a hill
C) a rock breaking upon impact
D) a rock sinking in the water
E) a rock warming in the sun
3) Chemistry is chiefly concerned with the study of which of the following types of changes in substances?
A) changes in volume
B) changes in composition
C) changes in location
D) changes in amount
E) changes in shape
4) What is the first step of the scientific method?
A) reaching a conclusion
B) stating a theory
C) formulating a hypothesis
D) making an observation
E) conducting an experiment
5) A hypothesis is _____ .
A) an observation recorded from an experiment
B) a thoroughly tested model
C) a descriptive model for observations
D) a concise statement that summarizes the results of a wide variety of experiments
6) Matter is defined as anything that _____ .
A) has a definite volume B) has mass and takes up space
C) can be weighed on a balance D) has a fixed volume and weight
7) A substance that forms a vapor is generally in what physical state at room temperature?
A) gas
B) liquid
C) plasma
D) solid
E) liquid or solid
8) Which state of matter takes both the shape and volume of its container?
A) solid B) liquid C) gas D) both B. and C.
9) Which state of matter is characterized by having a definite shape and a definite volume?
A) solid B) liquid C) plasma D) gas
10) Which of the following materials is a pure substance?
A) diamond B) brass C) tea D) air E) gasoline
11) All of the following are physical properties of matter EXCEPT _____.
A) melting point
B) color
C) hardness
D) explosiveness
E) mass
12) Which of the following is a physical change?
A) evaporation B) corrosion C) explosion D) food spoilage
13) Which of the following is NOT a pure substance?
A) liquid helium B) apple juice C) liquid oxygen D) mercury
14) Which of the following is a homogeneous mixture?
A) beef stew
B) soil
C) sand and water
D) brine
E) raisin bread
15) Which of the following is a true statement about homogeneous mixtures?
A) They consist of two or more phases.
B) They can consist only of liquids.
C) They have compositions that never vary.
D) They are known as solutions.
16) Which of the following is a true statement about compounds?
A) They have properties similar to those of their constituent elements.
B) They can be physically separated into their constituent elements.
C) They are pure substances.
D) They have variable compositions.
17) The chemical formula of a compound indicates the _____.
A) three-dimensional structure of the compound
B) identity of the elements in the compound only
C) relative proportions of the elements in the compound
D) type and arrangement of the bonds in the compound
18) What happens to the individual atoms in a chemical reaction?
A) Some are created.
B) Some are destroyed and some are created.
C) They are rearranged.
D) Some are destroyed.
19) Which of the following is true for all chemical reactions?
A) The total mass of the reactants increases.
B) Water is given off.
C) The total mass of the reactants equals the total mass of the products.
D) The total mass of the products is greater than the total mass of the reactants.
20) The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific notation?
A) 1.54 x 10-10 m B) 1.54 x 1010 m C) 1.54 x 10-12 m D) 1.54 x 1012 m
21) What is the result of multiplying (2.5 x 1010 ) x (3.5 x 10-7 )?
A) 8.75 x 1017 B) 8.75 x 103 C) 8.75 x 10-3 D) 8.75 x 10-17
22) When a test instrument is calibrated, does its accuracy, precision, or reliability improve?
A) accuracy B) reliability C) precision
23) In the measurement 0.503 L, which digit is the estimated digit?
A) 3
B) 5
C) the 0 to the left of the decimal point
D) the 0 immediately to the left of the 3
E) There is no estimated digit in this measurement.
24) How many significant figures are there in the measurement 40 500 mg?
A) two
B) five
C) four
D) three
E) This cannot be determined.
25) What is the measurement 1042 L rounded off to two significant digits?
A) 1050 L
B) 1.0 x 103L
C) 1040 L
D) 1.1 x 103 L
E) none of the above
26) Express the sum of 7.68 m and 5.0 m using the correct number of significant digits.
A) 12.7
B) 12.68
C) 13
D) 10 m
E) none of the above
27) Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.
A) 11 mm2
B) 10 mm2
C) 11.0 mm2
D) 11.00 mm2
E) none of the above
28) When multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the number of significant figures in _____ .
A) the most precise measurement.
B) all of the measurements.
C) the least precise measurement.
D) the least and most precise measurements.
29) What is the quantity 78 liters expressed in cubic meters?
A) 0.78 m3
B) 78 000 m3
C) 0.078 m3
D) 78 000 000 m3
E) 0.000 078 m3
30) If the temperature of a piece of steel decreases, what happens to its density?
A) The density decreases.
B) The density first increases, then decreases.
C) The density increases.
D) The density does not change.
E) The density first decreases, then increases.
31) What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
A) 479 mL B) 4.34 mL
C) 0.23 mL D) none of the above
32) The density is found by dividing _____.
A) volume by mass
B) mass by area
C) mass by length
D) area by mass
E) mass by volume
33) Which temperature scale has no negative temperatures?
A) Kelvin B) Celsius C) Fahrenheit D) Joule
34) What is the temperature of absolute zero measured in ¶C?
A) 0¶C B) -173¶C C) -73¶C D) -273¶C E) -373¶C
35) What is the boiling point in kelvins of water at 1 atmosphere of pressure?
A) 0 K B) 373 K C) 100 K D) 473 K E) 273 K
36) What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
A) 60.0 mL B) 42 mL C) 8.6 x 10 to power of (1) mL D) 0.012 mL
37) How many significant figures are there in the conversion factor 100 cm/1 m?
A) four
B) three
C) two
D) an unlimited number
E) one
38) On a typical day you inhale about 1 x 104 liters of air. What conversion factor would you use to express the volume in cubic centimeters?
A) 1.0 x 102 cm2/1 L B) 1 L/1.0 x 103 cm3 C) 1 L/1.0 x 102 cm3 D) 1.0 x 103 cm3/1 L
39) What is the result of converting 0.04 kmol to centimoles?
A) 0.4 cmol
B) 4000 cmol
C) 4 cmol
D) 40 cmol
E) 40 000 cmol
40) If 20 gits equal 1 erb, and 1 futz equals 2 hews, and 10 erbs equal 1 futz, how many gits equal 5 hews?
A) 1000 gits B) 100 gits C) 500 gits D) 50 gits
41) Express the density 5.6 g/cm3 in kg/m3.
A) 0.000 005 6 kg3/m
B) 5 600 000 kg/m3
C) 0.0056 kg/m3
D) 5600 kg/m3
E) 560 kg/m3
42) How would the rate 60 m/s be expressed in km/hr?
A) 216 km/hr
B) 2.16 km/hr
C) 0.216 km/hr
D) 21 600 km/hr
E) 0.002 16 km/hr
43) A blacksmith has to put new shoes on a stable of 20 horses. Each shoe requires 3 nails. How can he or she calculate the number of nails that must be brought to the stable?
A) number of nails x 4 shoes/3 nails x 1 horse/4 shoes =
B) number of horses x 4 shoes/1 horse x 3 nails/1 shoe =
C) number of nails x 1 shoe/nails x 3 nails/1 shoe =
D) number of shoes x 1 horse/4 shoes x 3 nails/1 horse =
44) What is the smallest particle of an element that retains the properties of that element?
A) an atom
B) a neutron
C) an electron
D) a proton
E) a molecule
45) Which of the following is NOT a part of Dalton's atomic theory?
A) Atoms that combine do so in simple whole-number ratios.
B) Atoms are always in motion.
C) Atoms of the same element are alike in mass and size.
D) All elements are composed of atoms.
46) What particles form the nucleus of an atom?
A) neutrons and electrons
B) electrons only
C) protons and neutrons
D) protons and electrons
E) None of the above
47) Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?
A) Cathode rays were always accompanied by anode rays.
B) An electron is 2000 times lighter than a hydrogen atom.
C) Cathode rays are negatively-charged particles.
D) Cathode rays can be deflected by magnets.
E) Cathode rays are always made of electrons, regardless of the gas used.
48) Which hypothesis led to the discovery of the proton?
A) A neutral atom should have dozens of subatomic particles.
B) Cathode rays should be attracted to a positively-charged plate.
C) When a neutral hydrogen atom loses an electron, a positively-charged particle should remain.
D) A proton should be 1840 times heavier than an electron.
E) The nucleus of an atom should contain neutrons.
49) Select the correct statement about subatomic particles.
A) The mass of a neutron nearly equals the mass of a proton.
B) Neutrons have no charge and are the lightest subatomic particle.
C) Electrons, protons, and neutrons all have the same mass.
D) Electrons are negatively charged and are the heaviest subatomic particle.
E) Protons are positively charged and the lightest subatomic particle.
50) As a consequence of the discovery of the nucleus by Rutherford, which model of the atoms is believed to be true?
A) A model in which the nucleus is made of neutrons only
B) A model in which the protons, electrons, and neutrons are evenly distributed throughout the volume of the atom
C) A model in which the nucleus is made of protons, electrons, and neutrons
D) A model in which the region outside the nucleus is largely empty space in which the electrons are situated
E) A model in which the nucleus is made of electrons and protons.
51) In which of the following sets are the symbol of the element, the number of protons, and the number of electrons given correctly?
A) Zn, 30 protons, 60 electrons
B) Cs, 55 protons, 132.9 electrons
C) In, 49 protons, 49 electrons
D) He, 4 protons, 4 electrons
E) F, 19 protons, 19 electrons
52) How are the number of neutrons in the nucleus of an atom calculated?
A) add the mass number to the number of electrons
B) add the number of electrons and protons together
C) subtract the number of protons from the mass number
D) subtract the number of electrons from the number of protons
53) The sum of the protons and neutrons in an atom equals the _____.
A) mass number B) nucleus number
C) atomic mass D) atomic number
54) Isotopes of the same element have different _____.
A) numbers of electrons
B) numbers of neutrons
C) numbers of protons
D) atomic numbers
E) symbols
55) Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 20 is 25% abundant; the isotope with a mass number of 22 is 75% abundant. What is the average atomic mass for element Z?
A) 42.0 g B) 20.5 g C) 2.0 g D) 21.5 g E) 21.0 g
56) The atomic mass of an element _____.
A) depends upon the number of isotopes of that element
B) depends upon the relative abundance of each isotope of the element
C) depends upon the mass of each isotope of that element
D) all of the above
57) What is each vertical column of elements in the periodic table called?
A) group or family B) list C) transition D) row
58) What type of ions have names ending in -ide?
A) only anions
B) only cations
C) only metalloid ions
D) only metal ions
E) only gaseous ions
59) What is the electrical charge of a cation?
A) a negative charge B) a positive charge
C) no charge D) None of the above
60) In which of the following sets is the number of electrons in each species the same?
A) F-, Cl-, Br-
B) Sr2+, Kr, Br-
C) Mg2+, O2-, Ne2+
D) Na+, K+, Rb+
E) Al3+, Cl-, Ar
61) In any chemical compound, the elements are always combined in the same proportion by _____.
A) density
B) mass
C) charge
D) volume
E) number of protons
62) The law of definite proportions applies to _____.
A) gases only
B) molecular compounds only
C) solids only
D) ionic compounds only
E) all compounds
63) Which of the following formulas represents an ionic compound?
A) N2O4 B) BaI2 C) Kr D) CS2 E) PCl3
64) Which of the following formulas represents a molecular compound?
A) BeF2 B) ZnO C) SO2 D) Mg3N2 E) Xe
65) In which of the following are the symbol and name for the ion given correctly?
A) NH+4: ammonia; H+ : hydride
B) OH- : hydroxide; O2-: oxide
C) PO with (superscript (cis_symbolcis_symbol) and: phosphate; PO with (superscript (cis_symbolcis_symbol) and: phosphite
D) HSO with (superscript (cis_symbolcis_symbol) and: bisulfate; HSO with (superscript (cis_symbolcis_symbol) and: bisulfite
E) C2H3O with (superscript (cis_symbolcis_symbol) and: acetate; C2O with (superscript (cis_symbolcis_symbol) and: oxalite
66) An -ate or -ite at the end of a compound name usually indicates that the compound contains _____.
A) only two elements
B) fewer anions than cations
C) a polyatomic ion
D) neutral molecules
E) hydroxide or cyanide ions
67) What is the correct formula for potassium sulfite?
A) KHSO3 B) K2SO4 C) K2S D) KHSO4 E) K2SO3
68) Which of the following compounds contains the lead(IV) ion?
A) PbO2 B) PbCl2 C) Pb2O D) PbO E) Pb4O3
69) Which set of chemical name and chemical formula for the same compound is correct?
A) tin(IV) bromide, SnBr4
B) aluminum fluorate, AlF3
C) beryllium sulfide, BeS2
D) iron(II) oxide, Fe2O3
E) potassium chloride, K2Cl2
70) Which set of chemical name and chemical formula for the same compound is correct?
A) iron(III) phosphate, FePO4
B) magnesium dichromate, MgCrO4
C) lithium carbonate, LiCO3
D) potassium chlorate, K2(ClO3)2
E) ammonium sulfite, (NH4)2S
71) Which of the following shows both the correct formula and correct name of an acid?
A) HClO2, chloric acid
B) HNO2, hydronitrous acid
C) H2CO3, bicarbonic acid
D) H3PO4, phosphoric acid
E) HI, iodic acid
72) Consider a mystery compound having the formula MxTy. If the compound is not an acid, if it contains only two elements and if M is not a metal; which of the following is true about the compound?
A) It contains a polyatomic ion.
B) Its name ends in -ic.
C) It is a binary molecular compound.
D) Its name ends in -ite or -ate.
E) It is a binary ionic compound.
73) What SI unit is used to measure the number of representative particles in a substance?
A) kilogram B) mole C) kelvin D) ampere E) candela
74) How many moles of tungsten atoms are there in 4.8 x 1025 atoms of tungsten?
A) 8.0 moles
B) 8.0 x 10 to power of (2) moles
C) 1.3 x 10 to power of (-2) moles
D) 8.0 x 10 to power of (1) moles
E) 1.3 x 10 to power of (-1) moles
75) How many moles of silver atoms are there in 1.8 x 1020 atoms of silver?
A) 3.0 x 10-4 B) 3.0 x 102 C) 1.1 x 1044 D) 3.3 x 10-3
76) How many ammonium ions, NH with (superscript (cis_symbolcis_symbol) and, are there in 5.0 mol (NH4)2S?
A) 6.0 x 1024 B) 3.0 x 1024 C) 1.5 x 1025 D) 6.0 x 1025 E) 3.4 x 102
77) Butanol is composed of carbon, hydrogen, and oxygen. If 1.0 mol of butanol contains 6.0 x 1024 atoms of hydrogen, what is the subscript for the hydrogen atom in C4H?O?
A) 6 B) 1 C) 8 D) 10 E) 4
78) How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O?
A) 35 x (6.02 x 1023) B) 5
C) 35 D) 5 x (6.02 x 1023)
79) Which of the following elements exists as a diatomic molecule?
A) aluminum B) neon C) nitrogen D) sulfur E) lithium
80) Which of the following is not a true statement concerning the gram atomic mass?
A) The gram atomic mass is the mass of 6.02 x 1023 atoms of any monatomic element.
B) The gram atomic mass is the mass of one mole of atoms.
C) The gram atomic mass is the number of grams of an element that is numerically equal to the atomic mass in amu.
D) The gram atomic mass is found by checking the periodic table.
E) The gram atomic mass is 12 g for magnesium.
81) What is the mass in grams of 5.90 mol C8H18?
A) 3.55 x 1024 g
B) 0.0512 g
C) 19.4 g
D) 673 g
E) 389 g
82) How many moles of CaBr2 are there in 5.0 grams of CaBr2?
A) 4.2 x 10-2 mol
B) 3.0 x 1024 mol
C) 2.5 x 10-2 mol
D) 1.0 x 103 mol
E) 4.0 x 101 mol
83) What is the percent composition of chromium in BaCrO4?
A) 20.5% B) 4.87% C) 54.2% D) 25.2% E) 9.47%
84) What is the mass of oxygen in 250 g of sulfuric acid, H2SO4?
A) 0.65 g B) 16 g C) 41 g D) 3.9 g E) 160 g
85) If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound?
A) 20.0% B) 44.4% C) 80.0% D) 55.6% E) 1.25%
86) What information is needed to calculate the percent composition of a compound?
A) the weight of the sample to be analyzed and its density
B) the density of the compound and Avogadro's number
C) the formula of the compound and the gram atomic mass of its elements
D) the formula of the compound and its density
E) the weight of the sample to be analyzed and its molar volume
87) What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?
A) SO2 B) SO C) S2O3 D) SO3 E) S6O4
88) What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?
A) C2H7N
B) CH4N7
C) C3HN2
D) C4H14N2
E) C4.5H15.5N2.2
89) Which of the following is NOT a true statement concerning empirical and molecular formulas?
A) The empirical formula of a compound can be triple its molecular formula.
B) Several compounds can have the same empirical formula, but have different molecular formulas.
C) If the molecular formula of hydrogen peroxide is H2O2, its empirical formula is HO.
D) The molecular formula of a compound can be some whole-number multiple of its empirical formula.
E) The molecular formula of a compound can be the same as its empirical formula.
90) What are the missing coefficients for the skeleton equation below?
Al2(SO4)3(aq) + KOH(aq) rightarrow Al(OH)3(aq) + K2SO4(aq)
A) 4,6,2,3 B) 2,3,1,1 C) 1,3,2,3 D) 2,12,4,6 E) 1,6,2,3
91) What are the missing coefficients for the skeleton equation below?
Cr(s) + Fe(NO3)2(aq) rightarrow Fe(s) + Cr(NO3)3(aq)
A) 4,6,6,2 B) 2,3,1,2 C) 1,3,3,1 D) 2,3,3,2 E) 2,3,2,3
92) When the equation, Fe + Cl2 rightarrow FeCl3, is balanced, what is the coefficient for Cl2?
A) 3 B) 4 C) 2 D) 1
93) Which of the following is NOT a true statement concerning what happens in all chemical reactions?
A) New atoms are formed as products.
B) The starting materials are named reactants.
C) The ways in which atoms are joined together are changed.
D) The bonds of the reactants are broken and new bonds of the products are formed.
E) In a word equation representing a chemical reaction, the reactants are written on the left and the products on the right.
94) A skeleton equation does NOT show which of the following?
A) the physical states of the substances
B) the reactants on the left, the products on the right
C) the relative amounts of reactants and products
D) the correct formulas of the reactants and products
E) an arrow connecting the reactants to the products
95) Chemical equations must be balanced to satisfy the _____.
A) law of conservation of mass B) principle of Avogadro
C) law of multiple proportions D) law of definite proportions
96) In every balanced chemical equation, each side of the equation has the same number of _____.
A) atoms
B) molecules
C) coefficients
D) subscripts
E) moles
97) When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is _____.
A) KOH + BaCl rightarrow KCl + BaOH
B) 2KOH + BaCl2 rightarrow 2KCl + Ba(OH)2
C) KOH + BaCl2 rightarrow KCl2 + BaOH
D) 2KOH + 2BaCl2 rightarrow 2KCl2 + 2Ba(OH)2
E) KH + BaCl rightarrow KCl + BaH
98) If a combination reaction takes place between potassium and chlorine, what is the product?
A) K2Cl B) KCl C) KCl2 D) PCl E) PCl2
99) Write a balanced equation to represent the decomposition of lead(IV) oxide.
A) 2PbO rightarrow 2Pb + O2
B) PbO2 rightarrow Pb + 2O
C) Pb2O rightarrow 2Pb + O
D) PbO2 rightarrow Pb + O2
E) PbO rightarrow Pb + O2
100) Which of the following statements is NOT true concerning the decomposition of a simple binary compound?
A) The reactant could be an ionic or a molecular compound.
B) The products are the constituent elements.
C) The reactant is a single substance.
D) The products are unpredictable.
E) Energy is usually required.
101) In a combustion reaction, one of the reactants is _____.
A) hydrogen
B) a metal
C) oxygen
D) a binary ionic compound
E) nitrogen
102) The calculation of quantities in chemical equations is called _____.
A) percent composition
B) stoichiometry
C) percent yield
D) dimensional analysis
E) accuracy and precision
103) What is conserved in the reaction shown below?
H2(g) + Cl2(g) Â 2HCl(g)
A) only mass, moles, and molecules
B) only mass, moles, molecules and volume
C) only mass
D) only mass and moles
104) In every chemical reaction, _____.
A) mass and molecules are conserved
B) moles and molecules are conserved
C) moles and liters are conserved
D) mass and atoms are conserved
E) mass and liters are conserved
105) Which of these is an INCORRECT interpretation of this balanced equation?
2S(s) + 3O2(g) Â 2SO3(g)
A) 2 mol S + 3 mol O2 Â 2 mol SO3
B) 2 g S + 3 g O2 Â 2 g SO3
C) 2 atoms S + 3 molecules O2 Â 2 molecules SO3
D) none of the above
106) How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s) Â 3Fe(s) + Al2O3(s)
A) 1.2 mol B) 1.6 mol C) 0.8 mol D) 4.8 mol E) 2.4 mol
107) How many moles of glucose, C6H12O6, can be "burned" biologically when 10.0 mol of oxygen is available?
C6H12O6(s) + 6O2(g) Â 6CO2(g) + 6H2O(l)
A) 301 mol B) 0.938 mol C) 1.67 mol D) 53.3 mol E) 60.0 mol
108) Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum?
2Al(s) + 3H2SO4(aq) Â Al2(SO4)3(aq) + 3H2(g)
A) 22.5 mol B) 2710 mol C) 10.0 mol D) 15.0 mol E) 0.100 mol
109) When glucose is consumed it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C6H12O6completely reacted with oxygen?
A) 66 g B) 12 000 g C) 11 g D) 1.8 g E) 1.5 g
110) How many moles of H3PO4 are produced when 71.0 g P4O10 reacts completely to form H3PO4?
P4O10(s) + 6H2O(l) Â 4H3PO4(aq)
A) 0.063 5 mol
B) 16.0 mol
C) 1.00 mol
D) 4.00 mol
E) 98.0 mol
111) The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO2 is formed?
2Pb(NO3)2(s) Â 2PbO(s) + 4NO2(g) + O2(g)
A) 2.00 g B) 32.0 g C) 2.88 g D) 1.00 g E) 46.0 g
112) How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water.)
Be(s) + 2H2O(l) Â Be(OH)2 (aq) + H2(g)
A) 4.00 g B) 648 g C) 162 g D) 324 g E) 36.0 g
113) Metallic copper is formed when aluminum reacts with copper(II) sulfate. How many grams of metallic copper can be obtained when 54.0 g of Al reacts with 319 g of CuSO4?
2Al + 3CuSO4 Â Al2(SO4)3 + 3Cu
A) 21.2 g B) 381 g C) 162 g D) 957 g E) 127 g
114) Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO3)2 is heated to give 5.5 g of PbO?
2Pb(NO3)2(s) Â 2PbO(s) + 4NO2(g) + O2(g)
A) 67% B) 56% C) 82% D) 44% E) 18%
115) When two substances react to form products, the reactant which is used up is called the _____.
A) limiting reagent
B) catalytic reagent
C) excess reagent
D) determining reagent
E) reactive reagent
116) When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the _____.
A) minimum yield
B) theoretical yield
C) percent composition
D) actual yield
E) percent yield
117) For a given chemical reaction, the theoretical yield is _____ greater than the actual yield.
A) always B) never C) sometimes
118) Which of the following is not a reason why actual yield is less than theoretical yield?
A) impure reactants present B) loss of product during purification
C) competing side reactions D) conservation of mass
119) How many joules are there in 148 calories? (1 cal = 4.18 J)
A) 6.61 J B) 35.4 J C) 148 J D) 3320 J E) 619 J
120) How much heat does it take to warm 16.0 g of pure water from 90.0¶C to 100.0¶C? (specific heat of water = 4.18 J/g x ¶C)
A) 66.9 joules B) 669 joules C) 16.0 joules D) 160 joules
121) When 45 g of an alloy is dropped into 100.0 g of water at 25¶C, the final temperature is 37¶C. What is the specific heat of the alloy?
A) 0.423 B) 9.88 C) 48.8 D) 1.77
122) What is the specific heat of olive oil if it takes approximately 420 J of heat to raise the temperature of 7 g of olive oil by 30¶C?
A) equal to the specific heat of water B) greater than the specific heat of water
C) less than the specific heat of water D) Not enough information given.
123) When cooking food with natural gas, the energy comes from _____.
A) kinetic energy in the gas
B) the volume of the gas
C) chemical potential energy of the gas molecules
D) the pressure of the gas
124) A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?
A) The temperature of the metal will increase.
B) The temperature of the water will increase and the temperature of the metal will decrease.
C) The temperature of the water will decrease.
D) The temperature of the water will decrease and the temperature of the metal will increase.
E) The temperature of the water will increase.
125) Two objects are sitting next to each other in direct sunlight. Object A gets hotter than object B.
A) Both objects have the same specific heat.
B) Object A has a higher specific heat than object B.
C) Object A has a lower specific heat than object B.
1) Answer: D
2) Answer: A
3) Answer: B
4) Answer: D
5) Answer: C
6) Answer: B
7) Answer: E
8) Answer: C
9) Answer: A
10) Answer: A
11) Answer: D
12) Answer: A
13) Answer: B
14) Answer: D
15) Answer: D
16) Answer: C
17) Answer: C
18) Answer: C
19) Answer: C
20) Answer: A
21) Answer: B
22) Answer: A
23) Answer: A
24) Answer: D
25) Answer: B
26) Answer: A
27) Answer: A
28) Answer: C
29) Answer: C
30) Answer: C
31) Answer: B
32) Answer: E
33) Answer: A
34) Answer: D
35) Answer: B
36) Answer: C
37) Answer: D
38) Answer: D
39) Answer: B
40) Answer: C
41) Answer: D
42) Answer: A
43) Answer: B
44) Answer: A
45) Answer: B
46) Answer: C
47) Answer: E
48) Answer: C
49) Answer: A
50) Answer: D
51) Answer: C
52) Answer: C
53) Answer: A
54) Answer: B
55) Answer: D
56) Answer: D
57) Answer: A
58) Answer: A
59) Answer: B
60) Answer: B
61) Answer: B
62) Answer: E
63) Answer: B
64) Answer: C
65) Answer: B
66) Answer: C
67) Answer: E
68) Answer: A
69) Answer: A
70) Answer: A
71) Answer: D
72) Answer: C
73) Answer: B
74) Answer: D
75) Answer: A
76) Answer: A
77) Answer: D
78) Answer: C
79) Answer: C
80) Answer: E
81) Answer: D
82) Answer: C
83) Answer: A
84) Answer: E
85) Answer: D
86) Answer: C
87) Answer: D
88) Answer: A
89) Answer: A
90) Answer: E
91) Answer: D
92) Answer: A
93) Answer: A
94) Answer: C
95) Answer: A
96) Answer: A
97) Answer: B
98) Answer: B
99) Answer: D
100) Answer: D
101) Answer: C
102) Answer: B
103) Answer: B
104) Answer: D
105) Answer: B
106) Answer: C
107) Answer: C
108) Answer: A
109) Answer: A
110) Answer: C
111) Answer: A
112) Answer: C
113) Answer: E
114) Answer: C
115) Answer: A
116) Answer: B
117) Answer: A
118) Answer: D
119) Answer: E
120) Answer: B
121) Answer: D
122) Answer: C
123) Answer: C
124) Answer: B
125) Answer: C
[edit]
[1/7/2002 2:02:28 PM | Mr. Fasciano]
The following questions are similar to questions on the final exam. You should work each one out and DON'T JUST MEMORIZE ANSWERS.
1. It is estimated that uranium is relatively common in the earth's crust, occurring in amounts of 4 g/metric ton.
A metric ton is 1000 kg. At this concentration, what mass of uranium is present in 1.0 mg of the earth's crust?
A) 4 nanograms
B) 4 micrograms
C) 4 milligrams
D) 4 ´ 10–5 g
E) 4 centigrams
2. Which of the following metric relationships is incorrect?
A) 1 microliter = 10–6 liters
B) 1 megagram = 106 grams
C) 1 millimeter = 103 meters
D) 1 kilogram = 103 grams
E) 100 centimeters = 1 meter
3. A set of tested hypotheses that gives an overall explanation of some natural phenomenon is called a(n)
A) observation.
B) measurement.
C) theory.
D) natural law.
E) experiment.
4. Express 784000000 in exponential notation.
A) 7.84 ´ 106
B) 7.84 ´ 108
C) 78.4 ´ 107
D) 784 ´ 106
E) 784 ´ 107
5. A titration was performed to find the concentration of hydrochloric acid with the following results:
Trial Molarity
1 1.25 ± 0.01
2 1.24 ± 0.01
3 1.26 ± 0.01
The actual concentration of HCl was determined to be 1.000 M; the results of the titration are:
A) both accurate and precise.
B) accurate but imprecise.
C) precise but inaccurate.
D) both inaccurate and imprecise.
E) accuracy and precision are impossible to determine with the available information.
6. The amount of uncertainty in a measured quantity is determined by:
A) both the skill of the observer and the limitations of the measuring instrument.
B) neither the skill of the observer nor the limitations of the measuring instrument.
C) the limitations of the measuring instrument only.
D) the skill of the observer only.
7. A scientist obtains the number 1250.37986 on a calculator. If this number actually has four (4) significant figures, how should it be written?
A) 1251
B) 1250.3799
C) 1250.4
D) 1.250 ´ 103
E) 1.250 ´ 10–3
8. How many significant figures are there in the number 0.0322?
A) 3
B) 5
C) 4
D) 2
E) 0
9. A piece of indium with a mass of 16.6 g is submerged in 46.3 cm3 of water in a graduated cylinder. The water level increases to 48.6 cm3. The correct value for the density of indium from these data is:
A) 7.217 g/cm3
B) 7.2 g/cm3
C) 0.14 g/cm3
D) 0.138 g/cm3
E) more than 0.1 g/cm3 away from any of these values.
10. A metric unit for mass is
A) pound.
B) kilogram.
C) ton.
D) ounce.
E) meter.
11. Using the rules of significant figures, calculate the following:
A) 17.5
B) 18
C) 17
D) 20
E) 17.48
12. Convert 974036 mm to km.
A) 9744036 km
B) 974.036 km
C) 974036000 km
D) 0.000974036 km
E) 0.974036 km
13. The volume of 65 L equals
A) 65 dm3
B) 65000 cm3
C) 650 dm3
D) 650 cm3
E) 65 dm3 and 65000 cm3
14. How many significant figures are there in the number 0.0006042?
A) 7
B) 3
C) 8
D) 4
E) 0
15. Convert 16.8 lb to g. (1 lb = 453.6 g)
A) 762.0 g
B) 3.70 ´ 104 g
C) 76.2 g
D) 7621 g
E) 7620 g
[edit]
[1/8/2002 1:34:27 PM | Mr. Fasciano]
1) The study of the composition and structure of matter is the domain of which field of science?
A) biology B) geology C) physics D) chemistry
2) Which of the following changes would be most appropriately considered in a study of chemistry, rather than any other science?
A) a rock melting as the result of being heated
B) a rock rolling down a hill
C) a rock breaking upon impact
D) a rock sinking in the water
E) a rock warming in the sun
3) Chemistry is chiefly concerned with the study of which of the following types of changes in substances?
A) changes in volume
B) changes in composition
C) changes in location
D) changes in amount
E) changes in shape
4) What is the first step of the scientific method?
A) reaching a conclusion
B) stating a theory
C) formulating a hypothesis
D) making an observation
E) conducting an experiment
5) A hypothesis is _____ .
A) an observation recorded from an experiment
B) a thoroughly tested model
C) a descriptive model for observations
D) a concise statement that summarizes the results of a wide variety of experiments
6) Matter is defined as anything that _____ .
A) has a definite volume B) has mass and takes up space
C) can be weighed on a balance D) has a fixed volume and weight
7) A substance that forms a vapor is generally in what physical state at room temperature?
A) gas
B) liquid
C) plasma
D) solid
E) liquid or solid
8) Which state of matter takes both the shape and volume of its container?
A) solid B) liquid C) gas D) both B. and C.
9) Which state of matter is characterized by having a definite shape and a definite volume?
A) solid B) liquid C) plasma D) gas
10) Which of the following materials is a pure substance?
A) diamond B) brass C) tea D) air E) gasoline
11) All of the following are physical properties of matter EXCEPT _____.
A) melting point
B) color
C) hardness
D) explosiveness
E) mass
12) Which of the following is a physical change?
A) evaporation B) corrosion C) explosion D) food spoilage
13) Which of the following is NOT a pure substance?
A) liquid helium B) apple juice C) liquid oxygen D) mercury
14) Which of the following is a homogeneous mixture?
A) beef stew
B) soil
C) sand and water
D) brine
E) raisin bread
15) Which of the following is a true statement about homogeneous mixtures?
A) They consist of two or more phases.
B) They can consist only of liquids.
C) They have compositions that never vary.
D) They are known as solutions.
16) Which of the following is a true statement about compounds?
A) They have properties similar to those of their constituent elements.
B) They can be physically separated into their constituent elements.
C) They are pure substances.
D) They have variable compositions.
17) The chemical formula of a compound indicates the _____.
A) three-dimensional structure of the compound
B) identity of the elements in the compound only
C) relative proportions of the elements in the compound
D) type and arrangement of the bonds in the compound
18) What happens to the individual atoms in a chemical reaction?
A) Some are created.
B) Some are destroyed and some are created.
C) They are rearranged.
D) Some are destroyed.
19) Which of the following is true for all chemical reactions?
A) The total mass of the reactants increases.
B) Water is given off.
C) The total mass of the reactants equals the total mass of the products.
D) The total mass of the products is greater than the total mass of the reactants.
20) The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific notation?
A) 1.54 x 10-10 m B) 1.54 x 1010 m C) 1.54 x 10-12 m D) 1.54 x 1012 m
21) What is the result of multiplying (2.5 x 1010 ) x (3.5 x 10-7 )?
A) 8.75 x 1017 B) 8.75 x 103 C) 8.75 x 10-3 D) 8.75 x 10-17
22) When a test instrument is calibrated, does its accuracy, precision, or reliability improve?
A) accuracy B) reliability C) precision
23) In the measurement 0.503 L, which digit is the estimated digit?
A) 3
B) 5
C) the 0 to the left of the decimal point
D) the 0 immediately to the left of the 3
E) There is no estimated digit in this measurement.
24) How many significant figures are there in the measurement 40 500 mg?
A) two
B) five
C) four
D) three
E) This cannot be determined.
25) What is the measurement 1042 L rounded off to two significant digits?
A) 1050 L
B) 1.0 x 103L
C) 1040 L
D) 1.1 x 103 L
E) none of the above
26) Express the sum of 7.68 m and 5.0 m using the correct number of significant digits.
A) 12.7
B) 12.68
C) 13
D) 10 m
E) none of the above
27) Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.
A) 11 mm2
B) 10 mm2
C) 11.0 mm2
D) 11.00 mm2
E) none of the above
28) When multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the number of significant figures in _____ .
A) the most precise measurement.
B) all of the measurements.
C) the least precise measurement.
D) the least and most precise measurements.
29) What is the quantity 78 liters expressed in cubic meters?
A) 0.78 m3
B) 78 000 m3
C) 0.078 m3
D) 78 000 000 m3
E) 0.000 078 m3
30) If the temperature of a piece of steel decreases, what happens to its density?
A) The density decreases.
B) The density first increases, then decreases.
C) The density increases.
D) The density does not change.
E) The density first decreases, then increases.
31) What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
A) 479 mL B) 4.34 mL
C) 0.23 mL D) none of the above
32) The density is found by dividing _____.
A) volume by mass
B) mass by area
C) mass by length
D) area by mass
E) mass by volume
33) Which temperature scale has no negative temperatures?
A) Kelvin B) Celsius C) Fahrenheit D) Joule
34) What is the temperature of absolute zero measured in ¶C?
A) 0¶C B) -173¶C C) -73¶C D) -273¶C E) -373¶C
35) What is the boiling point in kelvins of water at 1 atmosphere of pressure?
A) 0 K B) 373 K C) 100 K D) 473 K E) 273 K
36) What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
A) 60.0 mL B) 42 mL C) 8.6 x 10 to power of (1) mL D) 0.012 mL
37) How many significant figures are there in the conversion factor 100 cm/1 m?
A) four
B) three
C) two
D) an unlimited number
E) one
38) On a typical day you inhale about 1 x 104 liters of air. What conversion factor would you use to express the volume in cubic centimeters?
A) 1.0 x 102 cm2/1 L B) 1 L/1.0 x 103 cm3 C) 1 L/1.0 x 102 cm3 D) 1.0 x 103 cm3/1 L
39) What is the result of converting 0.04 kmol to centimoles?
A) 0.4 cmol
B) 4000 cmol
C) 4 cmol
D) 40 cmol
E) 40 000 cmol
40) If 20 gits equal 1 erb, and 1 futz equals 2 hews, and 10 erbs equal 1 futz, how many gits equal 5 hews?
A) 1000 gits B) 100 gits C) 500 gits D) 50 gits
41) Express the density 5.6 g/cm3 in kg/m3.
A) 0.000 005 6 kg3/m
B) 5 600 000 kg/m3
C) 0.0056 kg/m3
D) 5600 kg/m3
E) 560 kg/m3
42) How would the rate 60 m/s be expressed in km/hr?
A) 216 km/hr
B) 2.16 km/hr
C) 0.216 km/hr
D) 21 600 km/hr
E) 0.002 16 km/hr
43) A blacksmith has to put new shoes on a stable of 20 horses. Each shoe requires 3 nails. How can he or she calculate the number of nails that must be brought to the stable?
A) number of nails x 4 shoes/3 nails x 1 horse/4 shoes =
B) number of horses x 4 shoes/1 horse x 3 nails/1 shoe =
C) number of nails x 1 shoe/nails x 3 nails/1 shoe =
D) number of shoes x 1 horse/4 shoes x 3 nails/1 horse =
44) What is the smallest particle of an element that retains the properties of that element?
A) an atom
B) a neutron
C) an electron
D) a proton
E) a molecule
45) Which of the following is NOT a part of Dalton's atomic theory?
A) Atoms that combine do so in simple whole-number ratios.
B) Atoms are always in motion.
C) Atoms of the same element are alike in mass and size.
D) All elements are composed of atoms.
46) What particles form the nucleus of an atom?
A) neutrons and electrons
B) electrons only
C) protons and neutrons
D) protons and electrons
E) None of the above
47) Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?
A) Cathode rays were always accompanied by anode rays.
B) An electron is 2000 times lighter than a hydrogen atom.
C) Cathode rays are negatively-charged particles.
D) Cathode rays can be deflected by magnets.
E) Cathode rays are always made of electrons, regardless of the gas used.
48) Which hypothesis led to the discovery of the proton?
A) A neutral atom should have dozens of subatomic particles.
B) Cathode rays should be attracted to a positively-charged plate.
C) When a neutral hydrogen atom loses an electron, a positively-charged particle should remain.
D) A proton should be 1840 times heavier than an electron.
E) The nucleus of an atom should contain neutrons.
49) Select the correct statement about subatomic particles.
A) The mass of a neutron nearly equals the mass of a proton.
B) Neutrons have no charge and are the lightest subatomic particle.
C) Electrons, protons, and neutrons all have the same mass.
D) Electrons are negatively charged and are the heaviest subatomic particle.
E) Protons are positively charged and the lightest subatomic particle.
50) As a consequence of the discovery of the nucleus by Rutherford, which model of the atoms is believed to be true?
A) A model in which the nucleus is made of neutrons only
B) A model in which the protons, electrons, and neutrons are evenly distributed throughout the volume of the atom
C) A model in which the nucleus is made of protons, electrons, and neutrons
D) A model in which the region outside the nucleus is largely empty space in which the electrons are situated
E) A model in which the nucleus is made of electrons and protons.
51) In which of the following sets are the symbol of the element, the number of protons, and the number of electrons given correctly?
A) Zn, 30 protons, 60 electrons
B) Cs, 55 protons, 132.9 electrons
C) In, 49 protons, 49 electrons
D) He, 4 protons, 4 electrons
E) F, 19 protons, 19 electrons
52) How are the number of neutrons in the nucleus of an atom calculated?
A) add the mass number to the number of electrons
B) add the number of electrons and protons together
C) subtract the number of protons from the mass number
D) subtract the number of electrons from the number of protons
53) The sum of the protons and neutrons in an atom equals the _____.
A) mass number B) nucleus number
C) atomic mass D) atomic number
54) Isotopes of the same element have different _____.
A) numbers of electrons
B) numbers of neutrons
C) numbers of protons
D) atomic numbers
E) symbols
55) Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 20 is 25% abundant; the isotope with a mass number of 22 is 75% abundant. What is the average atomic mass for element Z?
A) 42.0 g B) 20.5 g C) 2.0 g D) 21.5 g E) 21.0 g
56) The atomic mass of an element _____.
A) depends upon the number of isotopes of that element
B) depends upon the relative abundance of each isotope of the element
C) depends upon the mass of each isotope of that element
D) all of the above
57) What is each vertical column of elements in the periodic table called?
A) group or family B) list C) transition D) row
58) What type of ions have names ending in -ide?
A) only anions
B) only cations
C) only metalloid ions
D) only metal ions
E) only gaseous ions
59) What is the electrical charge of a cation?
A) a negative charge B) a positive charge
C) no charge D) None of the above
60) In which of the following sets is the number of electrons in each species the same?
A) F-, Cl-, Br-
B) Sr2+, Kr, Br-
C) Mg2+, O2-, Ne2+
D) Na+, K+, Rb+
E) Al3+, Cl-, Ar
61) In any chemical compound, the elements are always combined in the same proportion by _____.
A) density
B) mass
C) charge
D) volume
E) number of protons
62) The law of definite proportions applies to _____.
A) gases only
B) molecular compounds only
C) solids only
D) ionic compounds only
E) all compounds
63) Which of the following formulas represents an ionic compound?
A) N2O4 B) BaI2 C) Kr D) CS2 E) PCl3
64) Which of the following formulas represents a molecular compound?
A) BeF2 B) ZnO C) SO2 D) Mg3N2 E) Xe
65) In which of the following are the symbol and name for the ion given correctly?
A) NH+4: ammonia; H+ : hydride
B) OH- : hydroxide; O2-: oxide
C) PO with (superscript (cis_symbolcis_symbol) and: phosphate; PO with (superscript (cis_symbolcis_symbol) and: phosphite
D) HSO with (superscript (cis_symbolcis_symbol) and: bisulfate; HSO with (superscript (cis_symbolcis_symbol) and: bisulfite
E) C2H3O with (superscript (cis_symbolcis_symbol) and: acetate; C2O with (superscript (cis_symbolcis_symbol) and: oxalite
66) An -ate or -ite at the end of a compound name usually indicates that the compound contains _____.
A) only two elements
B) fewer anions than cations
C) a polyatomic ion
D) neutral molecules
E) hydroxide or cyanide ions
67) What is the correct formula for potassium sulfite?
A) KHSO3 B) K2SO4 C) K2S D) KHSO4 E) K2SO3
68) Which of the following compounds contains the lead(IV) ion?
A) PbO2 B) PbCl2 C) Pb2O D) PbO E) Pb4O3
69) Which set of chemical name and chemical formula for the same compound is correct?
A) tin(IV) bromide, SnBr4
B) aluminum fluorate, AlF3
C) beryllium sulfide, BeS2
D) iron(II) oxide, Fe2O3
E) potassium chloride, K2Cl2
70) Which set of chemical name and chemical formula for the same compound is correct?
A) iron(III) phosphate, FePO4
B) magnesium dichromate, MgCrO4
C) lithium carbonate, LiCO3
D) potassium chlorate, K2(ClO3)2
E) ammonium sulfite, (NH4)2S
71) Which of the following shows both the correct formula and correct name of an acid?
A) HClO2, chloric acid
B) HNO2, hydronitrous acid
C) H2CO3, bicarbonic acid
D) H3PO4, phosphoric acid
E) HI, iodic acid
72) Consider a mystery compound having the formula MxTy. If the compound is not an acid, if it contains only two elements and if M is not a metal; which of the following is true about the compound?
A) It contains a polyatomic ion.
B) Its name ends in -ic.
C) It is a binary molecular compound.
D) Its name ends in -ite or -ate.
E) It is a binary ionic compound.
73) What SI unit is used to measure the number of representative particles in a substance?
A) kilogram B) mole C) kelvin D) ampere E) candela
74) How many moles of tungsten atoms are there in 4.8 x 1025 atoms of tungsten?
A) 8.0 moles
B) 8.0 x 10 to power of (2) moles
C) 1.3 x 10 to power of (-2) moles
D) 8.0 x 10 to power of (1) moles
E) 1.3 x 10 to power of (-1) moles
75) How many moles of silver atoms are there in 1.8 x 1020 atoms of silver?
A) 3.0 x 10-4 B) 3.0 x 102 C) 1.1 x 1044 D) 3.3 x 10-3
76) How many ammonium ions, NH with (superscript (cis_symbolcis_symbol) and, are there in 5.0 mol (NH4)2S?
A) 6.0 x 1024 B) 3.0 x 1024 C) 1.5 x 1025 D) 6.0 x 1025 E) 3.4 x 102
77) Butanol is composed of carbon, hydrogen, and oxygen. If 1.0 mol of butanol contains 6.0 x 1024 atoms of hydrogen, what is the subscript for the hydrogen atom in C4H?O?
A) 6 B) 1 C) 8 D) 10 E) 4
78) How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O?
A) 35 x (6.02 x 1023) B) 5
C) 35 D) 5 x (6.02 x 1023)
79) Which of the following elements exists as a diatomic molecule?
A) aluminum B) neon C) nitrogen D) sulfur E) lithium
80) Which of the following is not a true statement concerning the gram atomic mass?
A) The gram atomic mass is the mass of 6.02 x 1023 atoms of any monatomic element.
B) The gram atomic mass is the mass of one mole of atoms.
C) The gram atomic mass is the number of grams of an element that is numerically equal to the atomic mass in amu.
D) The gram atomic mass is found by checking the periodic table.
E) The gram atomic mass is 12 g for magnesium.
81) What is the mass in grams of 5.90 mol C8H18?
A) 3.55 x 1024 g
B) 0.0512 g
C) 19.4 g
D) 673 g
E) 389 g
82) How many moles of CaBr2 are there in 5.0 grams of CaBr2?
A) 4.2 x 10-2 mol
B) 3.0 x 1024 mol
C) 2.5 x 10-2 mol
D) 1.0 x 103 mol
E) 4.0 x 101 mol
83) What is the percent composition of chromium in BaCrO4?
A) 20.5% B) 4.87% C) 54.2% D) 25.2% E) 9.47%
84) What is the mass of oxygen in 250 g of sulfuric acid, H2SO4?
A) 0.65 g B) 16 g C) 41 g D) 3.9 g E) 160 g
85) If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound?
A) 20.0% B) 44.4% C) 80.0% D) 55.6% E) 1.25%
86) What information is needed to calculate the percent composition of a compound?
A) the weight of the sample to be analyzed and its density
B) the density of the compound and Avogadro's number
C) the formula of the compound and the gram atomic mass of its elements
D) the formula of the compound and its density
E) the weight of the sample to be analyzed and its molar volume
87) What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?
A) SO2 B) SO C) S2O3 D) SO3 E) S6O4
88) What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?
A) C2H7N
B) CH4N7
C) C3HN2
D) C4H14N2
E) C4.5H15.5N2.2
89) Which of the following is NOT a true statement concerning empirical and molecular formulas?
A) The empirical formula of a compound can be triple its molecular formula.
B) Several compounds can have the same empirical formula, but have different molecular formulas.
C) If the molecular formula of hydrogen peroxide is H2O2, its empirical formula is HO.
D) The molecular formula of a compound can be some whole-number multiple of its empirical formula.
E) The molecular formula of a compound can be the same as its empirical formula.
90) What are the missing coefficients for the skeleton equation below?
Al2(SO4)3(aq) + KOH(aq) rightarrow Al(OH)3(aq) + K2SO4(aq)
A) 4,6,2,3 B) 2,3,1,1 C) 1,3,2,3 D) 2,12,4,6 E) 1,6,2,3
91) What are the missing coefficients for the skeleton equation below?
Cr(s) + Fe(NO3)2(aq) rightarrow Fe(s) + Cr(NO3)3(aq)
A) 4,6,6,2 B) 2,3,1,2 C) 1,3,3,1 D) 2,3,3,2 E) 2,3,2,3
92) When the equation, Fe + Cl2 rightarrow FeCl3, is balanced, what is the coefficient for Cl2?
A) 3 B) 4 C) 2 D) 1
93) Which of the following is NOT a true statement concerning what happens in all chemical reactions?
A) New atoms are formed as products.
B) The starting materials are named reactants.
C) The ways in which atoms are joined together are changed.
D) The bonds of the reactants are broken and new bonds of the products are formed.
E) In a word equation representing a chemical reaction, the reactants are written on the left and the products on the right.
94) A skeleton equation does NOT show which of the following?
A) the physical states of the substances
B) the reactants on the left, the products on the right
C) the relative amounts of reactants and products
D) the correct formulas of the reactants and products
E) an arrow connecting the reactants to the products
95) Chemical equations must be balanced to satisfy the _____.
A) law of conservation of mass B) principle of Avogadro
C) law of multiple proportions D) law of definite proportions
96) In every balanced chemical equation, each side of the equation has the same number of _____.
A) atoms
B) molecules
C) coefficients
D) subscripts
E) moles
97) When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is _____.
A) KOH + BaCl rightarrow KCl + BaOH
B) 2KOH + BaCl2 rightarrow 2KCl + Ba(OH)2
C) KOH + BaCl2 rightarrow KCl2 + BaOH
D) 2KOH + 2BaCl2 rightarrow 2KCl2 + 2Ba(OH)2
E) KH + BaCl rightarrow KCl + BaH
98) If a combination reaction takes place between potassium and chlorine, what is the product?
A) K2Cl B) KCl C) KCl2 D) PCl E) PCl2
99) Write a balanced equation to represent the decomposition of lead(IV) oxide.
A) 2PbO rightarrow 2Pb + O2
B) PbO2 rightarrow Pb + 2O
C) Pb2O rightarrow 2Pb + O
D) PbO2 rightarrow Pb + O2
E) PbO rightarrow Pb + O2
100) Which of the following statements is NOT true concerning the decomposition of a simple binary compound?
A) The reactant could be an ionic or a molecular compound.
B) The products are the constituent elements.
C) The reactant is a single substance.
D) The products are unpredictable.
E) Energy is usually required.
101) In a combustion reaction, one of the reactants is _____.
A) hydrogen
B) a metal
C) oxygen
D) a binary ionic compound
E) nitrogen
102) The calculation of quantities in chemical equations is called _____.
A) percent composition
B) stoichiometry
C) percent yield
D) dimensional analysis
E) accuracy and precision
103) What is conserved in the reaction shown below?
H2(g) + Cl2(g) Â 2HCl(g)
A) only mass, moles, and molecules
B) only mass, moles, molecules and volume
C) only mass
D) only mass and moles
104) In every chemical reaction, _____.
A) mass and molecules are conserved
B) moles and molecules are conserved
C) moles and liters are conserved
D) mass and atoms are conserved
E) mass and liters are conserved
105) Which of these is an INCORRECT interpretation of this balanced equation?
2S(s) + 3O2(g) Â 2SO3(g)
A) 2 mol S + 3 mol O2 Â 2 mol SO3
B) 2 g S + 3 g O2 Â 2 g SO3
C) 2 atoms S + 3 molecules O2 Â 2 molecules SO3
D) none of the above
106) How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s) Â 3Fe(s) + Al2O3(s)
A) 1.2 mol B) 1.6 mol C) 0.8 mol D) 4.8 mol E) 2.4 mol
107) How many moles of glucose, C6H12O6, can be "burned" biologically when 10.0 mol of oxygen is available?
C6H12O6(s) + 6O2(g) Â 6CO2(g) + 6H2O(l)
A) 301 mol B) 0.938 mol C) 1.67 mol D) 53.3 mol E) 60.0 mol
108) Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum?
2Al(s) + 3H2SO4(aq) Â Al2(SO4)3(aq) + 3H2(g)
A) 22.5 mol B) 2710 mol C) 10.0 mol D) 15.0 mol E) 0.100 mol
109) When glucose is consumed it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C6H12O6completely reacted with oxygen?
A) 66 g B) 12 000 g C) 11 g D) 1.8 g E) 1.5 g
110) How many moles of H3PO4 are produced when 71.0 g P4O10 reacts completely to form H3PO4?
P4O10(s) + 6H2O(l) Â 4H3PO4(aq)
A) 0.063 5 mol
B) 16.0 mol
C) 1.00 mol
D) 4.00 mol
E) 98.0 mol
111) The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO2 is formed?
2Pb(NO3)2(s) Â 2PbO(s) + 4NO2(g) + O2(g)
A) 2.00 g B) 32.0 g C) 2.88 g D) 1.00 g E) 46.0 g
112) How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water.)
Be(s) + 2H2O(l) Â Be(OH)2 (aq) + H2(g)
A) 4.00 g B) 648 g C) 162 g D) 324 g E) 36.0 g
113) Metallic copper is formed when aluminum reacts with copper(II) sulfate. How many grams of metallic copper can be obtained when 54.0 g of Al reacts with 319 g of CuSO4?
2Al + 3CuSO4 Â Al2(SO4)3 + 3Cu
A) 21.2 g B) 381 g C) 162 g D) 957 g E) 127 g
114) Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO3)2 is heated to give 5.5 g of PbO?
2Pb(NO3)2(s) Â 2PbO(s) + 4NO2(g) + O2(g)
A) 67% B) 56% C) 82% D) 44% E) 18%
115) When two substances react to form products, the reactant which is used up is called the _____.
A) limiting reagent
B) catalytic reagent
C) excess reagent
D) determining reagent
E) reactive reagent
116) When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the _____.
A) minimum yield
B) theoretical yield
C) percent composition
D) actual yield
E) percent yield
117) For a given chemical reaction, the theoretical yield is _____ greater than the actual yield.
A) always B) never C) sometimes
118) Which of the following is not a reason why actual yield is less than theoretical yield?
A) impure reactants present B) loss of product during purification
C) competing side reactions D) conservation of mass
119) How many joules are there in 148 calories? (1 cal = 4.18 J)
A) 6.61 J B) 35.4 J C) 148 J D) 3320 J E) 619 J
120) How much heat does it take to warm 16.0 g of pure water from 90.0¶C to 100.0¶C? (specific heat of water = 4.18 J/g x ¶C)
A) 66.9 joules B) 669 joules C) 16.0 joules D) 160 joules
121) When 45 g of an alloy is dropped into 100.0 g of water at 25¶C, the final temperature is 37¶C. What is the specific heat of the alloy?
A) 0.423 B) 9.88 C) 48.8 D) 1.77
122) What is the specific heat of olive oil if it takes approximately 420 J of heat to raise the temperature of 7 g of olive oil by 30¶C?
A) equal to the specific heat of water B) greater than the specific heat of water
C) less than the specific heat of water D) Not enough information given.
123) When cooking food with natural gas, the energy comes from _____.
A) kinetic energy in the gas
B) the volume of the gas
C) chemical potential energy of the gas molecules
D) the pressure of the gas
124) A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?
A) The temperature of the metal will increase.
B) The temperature of the water will increase and the temperature of the metal will decrease.
C) The temperature of the water will decrease.
D) The temperature of the water will decrease and the temperature of the metal will increase.
E) The temperature of the water will increase.
125) Two objects are sitting next to each other in direct sunlight. Object A gets hotter than object B.
A) Both objects have the same specific heat.
B) Object A has a higher specific heat than object B.
C) Object A has a lower specific heat than object B.
1) Answer: D
2) Answer: A
3) Answer: B
4) Answer: D
5) Answer: C
6) Answer: B
7) Answer: E
8) Answer: C
9) Answer: A
10) Answer: A
11) Answer: D
12) Answer: A
13) Answer: B
14) Answer: D
15) Answer: D
16) Answer: C
17) Answer: C
18) Answer: C
19) Answer: C
20) Answer: A
21) Answer: B
22) Answer: A
23) Answer: A
24) Answer: D
25) Answer: B
26) Answer: A
27) Answer: A
28) Answer: C
29) Answer: C
30) Answer: C
31) Answer: B
32) Answer: E
33) Answer: A
34) Answer: D
35) Answer: B
36) Answer: C
37) Answer: D
38) Answer: D
39) Answer: B
40) Answer: C
41) Answer: D
42) Answer: A
43) Answer: B
44) Answer: A
45) Answer: B
46) Answer: C
47) Answer: E
48) Answer: C
49) Answer: A
50) Answer: D
51) Answer: C
52) Answer: C
53) Answer: A
54) Answer: B
55) Answer: D
56) Answer: D
57) Answer: A
58) Answer: A
59) Answer: B
60) Answer: B
61) Answer: B
62) Answer: E
63) Answer: B
64) Answer: C
65) Answer: B
66) Answer: C
67) Answer: E
68) Answer: A
69) Answer: A
70) Answer: A
71) Answer: D
72) Answer: C
73) Answer: B
74) Answer: D
75) Answer: A
76) Answer: A
77) Answer: D
78) Answer: C
79) Answer: C
80) Answer: E
81) Answer: D
82) Answer: C
83) Answer: A
84) Answer: E
85) Answer: D
86) Answer: C
87) Answer: D
88) Answer: A
89) Answer: A
90) Answer: E
91) Answer: D
92) Answer: A
93) Answer: A
94) Answer: C
95) Answer: A
96) Answer: A
97) Answer: B
98) Answer: B
99) Answer: D
100) Answer: D
101) Answer: C
102) Answer: B
103) Answer: B
104) Answer: D
105) Answer: B
106) Answer: C
107) Answer: C
108) Answer: A
109) Answer: A
110) Answer: C
111) Answer: A
112) Answer: C
113) Answer: E
114) Answer: C
115) Answer: A
116) Answer: B
117) Answer: A
118) Answer: D
119) Answer: E
120) Answer: B
121) Answer: D
122) Answer: C
123) Answer: C
124) Answer: B
125) Answer: C
[edit]
[1/7/2002 2:02:28 PM | Mr. Fasciano]
The following questions are similar to questions on the final exam. You should work each one out and DON'T JUST MEMORIZE ANSWERS.
1. It is estimated that uranium is relatively common in the earth's crust, occurring in amounts of 4 g/metric ton.
A metric ton is 1000 kg. At this concentration, what mass of uranium is present in 1.0 mg of the earth's crust?
A) 4 nanograms
B) 4 micrograms
C) 4 milligrams
D) 4 ´ 10–5 g
E) 4 centigrams
2. Which of the following metric relationships is incorrect?
A) 1 microliter = 10–6 liters
B) 1 megagram = 106 grams
C) 1 millimeter = 103 meters
D) 1 kilogram = 103 grams
E) 100 centimeters = 1 meter
3. A set of tested hypotheses that gives an overall explanation of some natural phenomenon is called a(n)
A) observation.
B) measurement.
C) theory.
D) natural law.
E) experiment.
4. Express 784000000 in exponential notation.
A) 7.84 ´ 106
B) 7.84 ´ 108
C) 78.4 ´ 107
D) 784 ´ 106
E) 784 ´ 107
5. A titration was performed to find the concentration of hydrochloric acid with the following results:
Trial Molarity
1 1.25 ± 0.01
2 1.24 ± 0.01
3 1.26 ± 0.01
The actual concentration of HCl was determined to be 1.000 M; the results of the titration are:
A) both accurate and precise.
B) accurate but imprecise.
C) precise but inaccurate.
D) both inaccurate and imprecise.
E) accuracy and precision are impossible to determine with the available information.
6. The amount of uncertainty in a measured quantity is determined by:
A) both the skill of the observer and the limitations of the measuring instrument.
B) neither the skill of the observer nor the limitations of the measuring instrument.
C) the limitations of the measuring instrument only.
D) the skill of the observer only.
7. A scientist obtains the number 1250.37986 on a calculator. If this number actually has four (4) significant figures, how should it be written?
A) 1251
B) 1250.3799
C) 1250.4
D) 1.250 ´ 103
E) 1.250 ´ 10–3
8. How many significant figures are there in the number 0.0322?
A) 3
B) 5
C) 4
D) 2
E) 0
9. A piece of indium with a mass of 16.6 g is submerged in 46.3 cm3 of water in a graduated cylinder. The water level increases to 48.6 cm3. The correct value for the density of indium from these data is:
A) 7.217 g/cm3
B) 7.2 g/cm3
C) 0.14 g/cm3
D) 0.138 g/cm3
E) more than 0.1 g/cm3 away from any of these values.
10. A metric unit for mass is
A) pound.
B) kilogram.
C) ton.
D) ounce.
E) meter.
11. Using the rules of significant figures, calculate the following:
A) 17.5
B) 18
C) 17
D) 20
E) 17.48
12. Convert 974036 mm to km.
A) 9744036 km
B) 974.036 km
C) 974036000 km
D) 0.000974036 km
E) 0.974036 km
13. The volume of 65 L equals
A) 65 dm3
B) 65000 cm3
C) 650 dm3
D) 650 cm3
E) 65 dm3 and 65000 cm3
14. How many significant figures are there in the number 0.0006042?
A) 7
B) 3
C) 8
D) 4
E) 0
15. Convert 16.8 lb to g. (1 lb = 453.6 g)
A) 762.0 g
B) 3.70 ´ 104 g
C) 76.2 g
D) 7621 g
E) 7620 g
[edit]
[12/13/2001 3:26:37 PM | Mr. Fasciano]
The next major exam is a week from today, Dec 20, 2001.
This exam primarily covers chapters 8 and 9. There will be some review on the test. Primarily naming chemical compounds from their formula and vice versa. You also must be able to balance reactions.
STUDY GUIDE FOR EXAM 4
1. Know the definition of AMU and be able to convert from amu to grams and vice versa.
2. Be able to calculate the average ATOMIC MASS from a weighted average the isotopes given percent abundances.
3. Be able to convert from mass to moles to molecules to atoms and vice versa.
4. Be able to calculate the molar mass of a compound using the periodic table.
5. Be able to calculate the empirical and molecular formulas given either the % composition or the masses of the individual elements.
6. Be able to interpret the molecular and mass information given in a balanced chemical equation.
7. Be able to use a balanced chemical equation to determine the molar relationships between reactants and products.
8. Understand the relationship between masses of reactants and products in a chemical equation.
9. Be able to recognize (figure out) the LIMITING REACTANT in a chemical reaction.
10. Given the masses of the reactants be able to find the masses of all the products and masses of any leftover reactant.
11. Be able to determine the PERCENT YIELD in a chemical reaction given the actual amount produced and the mass of the reactants.
START STUDYING NOW!!!!!!!!!!!!!!! START STUDYING NOW!!!!!!!!!!!!!!!START STUDYING NOW!!!!!!!!!!!!!START STUDYING NOW!!!!!!!!!!!!!!!!!!
[edit]
[12/13/2001 1:50:54 PM | Mr. Fasciano]
Stoichiometry of Magnesium Oxide Lab.
Answers to pre-lab questions:
1. a) % Mg = 60.3 %
b) % O = 39.7 %
2. 3.37 g
3. 93.5%
[edit]
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