Posted by **Jayd** on Thursday, May 10, 2007 at 7:13pm.

The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is 0.300 atm in a mixture of the two gases.

a) What is the mole fraction of each gas in the mixture?

b) If the mixture occupies a volume of 11.5 L at 65 degress C, calculate the total number of moles of gas in the mixture.

a) partial pressure CH4 = 0.185 atm.

partial pressure O2 = 0.300

total pressure = 0.185 + 0.300

X=mol fraction CH4 = pressure CH4/total pressure.

X=mol fraction O2 = pressure O2/total pressure.

b)Use PV = nRT

Use total P, you have V, n is what you solve for, R is the gas constant (0.08205 L*atm/mol*K) and T is 65 (don't forget to change to Kelvin). Using total pressure will get total n.

- Chemsitry II -
**Anonymous**, Monday, October 31, 2011 at 10:49pm
.201

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