61. A sample of oxygen of mass 25.0 g is confi ned in a vessel at 0°C and 1000. torr. Then 6.00 g of hydrogen is pumped
into the vessel at constant temperature. What will be the
fi nal pressure in the vessel (assuming only mixing with no
62. A gaseous mixture contains 3.23 g of chloroform,
CHCl3, and 1.22 g of methane, CH4. Assuming that both
compounds remain as gases, what pressure is exerted by
the mixture inside a 50.0-mL metal container at 275°C?
What pressure is contributed by the CHCl3?
69. ▲ A study of climbers who reached the summit of Mt.
Everest without supplemental oxygen revealed that the
partial pressures of O2 and CO2 in their lungs were 35
torr and 7.5 torr, respectively. The barometric pressure at
the summit was 253 torr. Assume that the lung gases are
saturated with moisture at a body temperature of 37°C.
Calculate the partial pressure of inert gas (mostly nitrogen) in the climbers’ lungs.
72. During a collision, automobile air bags are inflated
by the N2 gas formed by the explosive decomposition of
sodium azide, NaN3.
2NaN3 --> 2Na + 3N2
What mass of sodium azide would be needed to inflate a
25.0-L bag to a pressure of 1.40 atm at 25°C?
75. ■ Calculate the volume of methane, CH4, measured at
300. K and 825 torr, that can be produced by the bacterial
breakdown of 1.10 kg of a simple sugar.
C6H12O6 --> 3CH4 + 3CO2
79. ■ We burn 12.50 L of ammonia in 20.00 L of oxygen at
500.°C. What volume of nitric oxide, NO, gas can form?
What volume of steam, H2O(g), is formed? Assume that
all gases are at the same temperature and pressure, and
that the limiting reactant is used up.
4NH3 (g) + 5O2 (g) --> 4NO(g) + 6H2O(g)
107. A particular tank can safely hold gas up to a pressure
of 44.3 atm. When the tank contains 38.1 g of N2 at
25°C, the gas exerts a pressure of 10.1 atm. What is the
highest temperature to which the gas sample can be
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