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1. What is the mass, in grams, of one copper atom?
A. 1.055 ´ 10-22 g
B. 63.55 g
C. 1 amu
D. 1.66 ´ 10-24 g
E. 9.476 ´ 1021 g

9. Hydrochloric acid can be prepared by the following reaction:

2NaCl(s) + H2SO4(aq) ® 2HCl(g) + Na2SO4(s)

How many grams of HCl can be prepared from 2.00 mol H2SO4 and 150 g NaCl?

A. 7.30 g
B. 93.5 g
C. 146 g
D. 150 g
E. 196 g

10. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below?
2Al + Cr2O3 ® Al2O3 + 2Cr
A. 7.7 g
B. 15.4 g
C. 27.3 g
D. 30.8 g
E. 49.9 g

12.
At what temperature does the numerical reading on a Celsius thermometer equal that on a Fahrenheit thermometer?

A)
0 °C

B)
–40 °C

C)
100 °C

D)
–32 °C

22. Ammonia boils at -33.4°C. What temperature is this in °F?
A. -60.1°F
B. -92.1°F
C. -28.1°F
D. +13.5°F

43. Which of these pairs of elements would be most likely to form a molecular compound?
A. Na and Br
B. Ca and O
C. C and O
D. Zn and O
E. Mg and Cl

69. Which of the following samples contains the greatest number of atoms?
A. 100 g of Pb
B. 2.0 mole of Ar
C. 0.1 mole of Fe
D. 5 g of He
E. 20 million O2 molecules

75. Hydrochloric acid can be prepared by the following reaction:

2NaCl(s) + H2SO4(aq) ® 2HCl(g) + Na2SO4(s)

How many grams of HCl can be prepared from 2.00 mol H2SO4 and 150 g NaCl?
A. 7.30 g
B. 93.5 g
C. 146 g
D. 150 g
E. 196 g

76. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below?
2Al + Cr2O3 ® Al2O3 + 2Cr
A. 7.7 g
B. 15.4 g
C. 27.3 g
D. 30.8 g
E. 49.9 g

78.
Consider the combustion of carbon monoxide (CO) in oxygen gas:
2CO(g) + O2(g) 2CO2(g)
Starting with 3.60 moles of CO, calculate the number of moles of CO2 produced if there is enough oxygen gas to react with all of the CO.

A)
7.20 mol

B)
44.0 mol

C)
3.60 mol

D)
1.80 mol

79.
Nitrous oxide (N2O) is also called “laughing gas.” It can be prepared by the thermal decomposition of ammonium nitrate (NH4NO3). The other product is H2O. The balanced equation for this reaction is:
NH4NO3 N2O + 2H2O
How many grams of N2O are formed if 0.46 mole of NH4NO3 is used in the reaction?

A)
2.0 g

B)
3.7 ˟101 g

C)
2.0 ˟101 g

D)
4.6 ˟ 10-1 g

80.
Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark-brown gas:
2NO(g) + O2(g) 2NO2(g)
In one experiment 0.886 mole of NO is mixed with 0.503 mole of O2. Calculate the number of moles of NO2 produced (note: first determine which is the limiting reagent).

A)
0.886 mol

B)
0.503 mol

C)
1.01 mol

D)
1.77 mol

81.
The fertilizer ammonium sulfate [(NH4)2SO4] is prepared by the reaction between ammonia (NH3) and sulfuric acid:
2NH3(g) + H2SO4(aq) (NH4)2SO4(aq)
How many kilograms of NH3 are needed to produce 1.00 ´ 105 kg of (NH4)2SO4?

A)
1.70 ˟ 104 kg

B)
3.22 ˟ 103 kg

C)
2.58 ˟ 104 kg

D)
7.42 ˟ 104 kg

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