MCA Quarter 3 Multiple Choice Review
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
____
____
____
____
____
____
____
____
____
____
1. What SI unit is used to measure the number of representative particles in a substance?
a. kilogram
c. kelvin
b. ampere
d. mole
2. Which of the following elements exists as a diatomic molecule?
a. neon
c. nitrogen
b. lithium
d. sulfur
3. Avogadro's number of representative particles is equal to one ____.
a. kilogram
c. kelvin
b. gram
d. mole
4. How many moles of tungsten atoms are in 4.8 10 atoms of tungsten?
a. 8.0 10 moles
c. 1.3 10 moles
b. 8.0 10 moles
d. 1.3 10 moles
5. How many atoms are in 3.5 moles of arsenic atoms?
a. 5.8 10 atoms
c. 2.1 10 atoms
b. 7.5 10 atoms
d. 1.7 10 atoms
6. Butanol is composed of carbon, hydrogen, and oxygen. If 1.0 mol of butanol contains 6.0 10 atoms of
hydrogen, what is the subscript for the hydrogen atom in C H O?
a. 1
c. 6
b. 10
d. 8
7. The atomic masses of any two elements contain the same number of ____.
a. atoms
c. ions
b. grams
d. milliliters
8. What is true about the molar mass of chlorine gas?
a. The molar mass is 35.5 g.
b. The molar mass is 71.0 g.
c. The molar mass is equal to the mass of one mole of chlorine atoms.
d. none of the above
9. The mass of a mole of NaCl is the ____.
a. molar mass
c. molecular mass
b. atomic mass
d. gram atomic mass
10. What is the molar mass of AuCl3?
a. 96 g
c. 232.5 g
b. 130 g
d. 303.6 g
11. The molar mass of C H and the molar mass of CaCO contain approximately the same number of ____.
a. carbon atoms
c. cations
b. anions
d. grams
____ 12. For which of the following conversions does the value of the conversion factor depend upon the formula of
the substance?
a. volume of gas (STP) to moles
b. density of gas (STP) to molar mass
c. mass of any substance to moles
d. moles of any substance to number of particles
____ 13. The volume of one mole of a substance is 22.4 L at STP for all ____.
a. gases
c. solids
b. liquids
d. compounds
____ 14. The molar volume of a gas at STP occupies ____.
a. 22.4 L
c. 1 kilopascal
b. 0 C
d. 12 grams
____ 15. The molar mass of a substance can be calculated from its density alone, if that substance is a(n) ____.
a. element
c. liquid
b. gas at STP
d. solid
____ 16. The molar mass of a gas can be determined from which of the following?
a. the density of the gas at STP
c. Avogadro's number
b. the volume of a mole of the gas
d. none of the above
____ 17. What is the number of moles in 500 L of He gas at STP?
a. 0.05 mol
c. 22 mol
b. 0.2 mol
d. 90 mol
____ 18. To determine the formula of a new substance, one of the first steps is to find the ____.
a. molar mass
c. volume at STP
b. percent composition
d. number of particles per mole
____ 19. 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 weight of the sample to be analyzed and its molar volume
c. the formula of the compound and the atomic mass of its elements
d. the formula of the compound and its density
____ 20. What is the percent by mass of carbon in acetone, C H O?
a. 20.7%
c. 1.61%
b. 62.1%
d. 30.0%
____ 21. The lowest whole-number ratio of the elements in a compound is called the ____.
a. empirical formula
c. binary formula
b. molecular formula
d. representative formula
____ 22. Chemical reactions ____.
a. occur only in living organisms
c. only occur outside living organisms
b. create and destroy atoms
d. produce new substances
____ 23. Everyday equations describe ____.
a. thermonuclear reactions
c. chemical reactions
b. everyday processes
d. biological chemistry
____ 24. What does the symbol in a chemical equation mean?
a. Heat is supplied to the reaction.
c. yields
b. A catalyst is needed.
d. precipitate
____ 25. Chemical equations ____.
a. describe chemical reactions
b. show how to write chemical formulas
c. give directions for naming chemical compounds
d. describe only biological changes
____ 26. Symbols used in equations, together with the explanations of the symbols, are shown below. Which set is
correct?
a. (g), grams
c. (aq), dissolved in water
b. (l), liters
d. s, solid product
____ 27. This symbol (
) indicates that ____.
a. heat must be applied
b. an incomplete combustion reaction has occurred
c. a gas is formed by the reaction
d. the reaction is reversible
____ 28. A catalyst is ____.
a. the product of a combustion reaction
b. not used up in a reaction
c. one of the reactants in single-replacement reactions
d. a solid product of a reaction
____ 29. What are the coefficients that will balance the skeleton equation below?
AlCl + NaOH
Al(OH)
NaCl
a. 1, 3, 1, 3
c. 1, 1, 1, 3
b. 3, 1, 3, 1
d. 1, 3, 3, 1
____ 30. Chemical equations must be balanced to satisfy ____.
a. the law of definite proportions
c. the law of conservation of mass
b. the law of multiple proportions
d. Avogadro’s principle
____ 31. In every balanced chemical equation, each side of the equation has the same number of ____.
a. atoms of each element
c. moles
b. molecules
d. coefficients
____ 32. In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that
shows the ____.
a. periodic table
b. activity series of metals
c. common polyatomic ions
d. ionic charges of representative elements
____ 33. In a combustion reaction, one of the reactants is ____.
a. hydrogen
c. oxygen
b. nitrogen
d. a metal
____ 34. The type of reaction that takes place when one element reacts with a compound to form a new compound and
a different element is a ____.
a. combination reaction
c. single-replacement reaction
b. decomposition reaction
d. double-replacement reaction
____ 35. In a double-replacement reaction, the ____.
a. products are always molecular
b. reactants are two ionic compounds
c. reactants are two elements
d. products are a new element and a new compound
____ 36. Which of the following statements is true about single-replacement reactions?
a. They are restricted to metals.
c. Two reactants produce two products.
b. They involve a single product.
d. Any metal replaces any other metal.
____ 37. In the activity series of metals, which metal(s) will displace hydrogen from an acid?
a. only metals above hydrogen
c. any metal
b. only metals below hydrogen
d. only metals from Li to Na
____ 38. In a double-replacement reaction, ____.
a. the reactants are usually a metal and a nonmetal
b. one of the reactants is often water
c. the reactants are generally two ionic compounds in aqueous solution
d. energy in the form of heat or light is often produced
____ 39. The calculation of quantities in chemical equations is called ____.
a. stoichiometry
c. percent composition
b. dimensional analysis
d. percent yield
____ 40. What is conserved in the reaction shown below?
H (g) + Cl (g)  2HCl(g)
a. mass only
c. mass, moles, and molecules only
b. mass and moles only
d. mass, moles, molecules, and volume
____ 41. What is conserved in the reaction shown below?
N (g) + 3F (g)  2NF (g)
a. atoms only
c. mass and atoms only
b. mass only
d. moles only
____ 42. In every chemical reaction, ____.
a. mass and molecules are conserved
c. mass and atoms are conserved
b. moles and liters are conserved
d. moles and molecules are conserved
____ 43. In a chemical reaction, the mass of the products ____.
a. is less than the mass of the reactants
b. is greater than the mass of the reactants
c. is equal to the mass of the reactants
d. has no relationship to the mass of the reactants
____ 44. In any chemical reaction, the quantities that are preserved are ____.
a. the number of moles and the volumes
b. the number of molecules and the volumes
c. mass and number of atoms
d. mass and moles
____ 45. The first step in most stoichiometry problems is to ____.
a. add the coefficients of the reagents
c. convert given quantities to volumes
b. convert given quantities to moles
d. convert given quantities to masses
____ 46. Which type of stoichiometric calculation does not require the use of the molar mass?
a. mass-mass problems
c. mass-particle problems
b. mass-volume problems
d. volume-volume problems
____ 47. When two substances react to form products, the reactant which is used up is called the ____.
a. determining reagent
c. excess reagent
b. limiting reagent
d. catalytic reagent
____ 48. 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. actual yield
c. theoretical yield
b. percent yield
d. minimum yield
MULTIPLE CHOICE
MCA Quarter 3 Multiple Choice Review
Answer Section
MULTIPLE CHOICE
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
D
C
D
B
10.1.2
C
10.1.2
B
10.1.2
A
B
A
D
10.1.4
D
10.1.4
C
A
A
B
A
C
B
C
B
A
D
B
A
A
C
D
B
A
11.1.3
C
A
11.1.3
B
DIF:
DIF:
DIF:
DIF:
L1
L1
L1
L2
REF:
REF:
REF:
REF:
p. 290
OBJ: 10.1.2
p. 290
OBJ: 10.1.2
p. 290
OBJ: 10.1.2
p. 290, p. 291
DIF: L2
REF: p. 291, p. 292
DIF: L3
REF: p. 290, p. 291
DIF:
DIF:
DIF:
DIF:
REF:
REF:
REF:
REF:
L1
L2
L1
L2
p. 294
OBJ: 10.1.3
p. 294
OBJ: 10.1.3
p. 295
OBJ: 10.1.4
p. 295, p. 296
DIF: L2
REF: p. 295, p. 296
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
L2
L1
L1
L1
L1
L2
L1
L1
L2
L1
L1
L1
L1
L1
L1
L1
L1
L1
p. 297
p. 300
p. 300
p. 302
p. 302
p. 301
p. 305
p. 307
p. 307
p. 309
p. 321
p. 324
p. 323
p. 323
p. 323
p. 323
p. 323
p. 324, p. 325
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
10.2.1
10.2.2
10.2.2
10.2.2
10.2.2
10.2.2
10.3.1
10.3.1
10.3.1
10.3.2
11.1.1
11.1.1
11.1.2
11.1.2
11.1.2
11.1.2
11.1.2
DIF: L1
DIF: L1
REF: p. 325
OBJ: 11.1.3
REF: p. 325, p. 327
DIF: L1
REF: p. 333
OBJ: 11.2.1
33. ANS: C
34. ANS: C
35. ANS: B
OBJ: 11.2.1
36. ANS: C
OBJ: 11.2.1
37. ANS: A
38. ANS: C
OBJ: 11.2.1
39. ANS: A
40. ANS: D
41. ANS: C
42. ANS: C
43. ANS: C
44. ANS: C
45. ANS: B
46. ANS: D
47. ANS: B
48. ANS: C
DIF: L1
DIF: L1
DIF: L1
REF: p. 336
OBJ: 11.2.1
REF: p. 333
OBJ: 11.2.1
REF: p. 334, p. 335
DIF: L2
REF: p. 333, p. 334
DIF: L2
DIF: L2
REF: p. 333
OBJ: 11.2.1
REF: p. 334, p. 335
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
L1
L1
L1
L1
L1
L1
L1
L1
L1
L1
p. 354
p. 356
p. 356
p. 356
p. 356
p. 356
p. 356
p. 365
p. 369
p. 372
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
12.1.1
12.1.2
12.1.2
12.1.2
12.1.2
12.1.2
12.1.2
12.2.2
12.3.1
12.3.2