1-A mixture containing 13.5 g of oxygen and 60.4 g
of N2 exerts a pressure of 2.13 atm at 25°C. What is the volume of the container, and
what are the partial pressures of each gas?
2-A mixture of SO2(g) and SO3(g) is to be prepared
with a total pressure of 1.4 atm. If the mole fractions of the gases are 0.70 and 0.30,
respectively, what are the partial pressures? If the mixture is to occupy 2.50 L at 27°C,
what mass of each gas is needed?
3-Suppose that 270 mL of CO2 at 1.03 atm and 25°C
is produced by this reaction. Assuming that an excess of hydrochloric acid was pres-
ent, how many grams of sodium bicarbonate were used?
4-SO2 can be generated in the laboratory by heating
ZnS with O2. (The other product is zinc oxide.) If 14.5 L of oxygen at STP is reacted
with excess zinc sulf de, what volume of SO2 at STP is generated?
5-Under less extreme conditions, the corrections for
nonideal behavior are smaller. Calculate the pressure of 0.500 mol of methane occupying
15.0 L at 25.7°C using both the ideal gas law and the van der Waals equation. Compare
the percentage correction with that calculated in the example above.
6-Calculate the enthalpy change when 14.5 g of water
vapor condenses to liquid water.
7-Use the following thermochemical equations as
needed to f nd the heat of formation of diamond:
C(diamond) + O2(g) : CO2(g) DH° = –395.4 kJ
2 CO2(g) : 2 CO(g) + O2 (g) DH° = 566.0 kJ
C(graphite) + O2(g) : CO2(g) DH° = –393.5 kJ
2 CO(g) : C(graphite) + CO2(g) DH° = –172.5 kJ
8-Use heat of formation data from Appendix E to
calculate DH ° for the following reaction: ClO2(g) + O(g) : ClO(g) + O2(g)
9-If 124 kJ of heat is absorbed in a reaction that forms
nitric oxide from nitrogen and oxygen, what mass of NO must have been produced?
What mass of N2 was consumed?
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