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7. A container has a volume of 3.2 m3 at 88 oC and a mixture of gases containing 1.5 grams of H2, 85.2 grams of O2, and 17 .0 grams of Ar.
First, what is the partial pressure of hydrogen gas? Secondly, what is the total pressure in the vessel?
ans. partial pressure H2 = 6.9 x 10-3 atm
and PT = 3.54 x 10-2 atm

A. Determine the partial pressure H2
Given:  Since hydrogen is a gas and the mass, volume, and temperature of the gas is known; we can utilize the ideal gas law to determine the individual pressure do to H2 . In order to determine the partial pressure H2, we will use the ideal gas law.


1. We assume this equation is valid given the temperature is moderately high.
2. To utilize this equation the mass of H2 must be changed to gram-moles.
3. Conver Temperature from celcius to Kelvin.
4. Convert Volume from cubic meters to Liters.

Know:

1 mole of H2 ~ 2  grams H2                  K = C + 273?
100 cm ~ 1 meter                                      1000 cm3 ~ 1 Liter

A. Determine the total pressure, PT
B. Given: The vessel contains a mixture of three gases.
Know: Daltons Law of Partial Pressure:

Since mass of all three gases, volume, and temperature of the gases are given; we can utilize the ideal gas law to determine the individual pressure do to Ar, H2, and O2 . In order to determine the partial pressures of Ar and O2, we will use same approach we did for determining the partial pressure of H2.