A container encloses 3.7 mol of an ideal gas that has molar M_1 mass and 0.30 mo

Question

A container encloses 3.7 mol of an ideal gas that has molar M_1 mass and 0.30 mol of a second gas that has a molar mass of M_2 = 4.4M_1 What fraction of the total pressure on the container wall is attributable to the second gas? (The kinetic theory explanation of pressure leads to the experimentally discovered law of partial pressures for a mixture of gases that do not react chemically: The total pressure exerted by the mixture is equal to the sum of the pressures that the several gases would exert separately if each were to occupy the vessel alone.)

Explanation / Answer

P1 = n1RT/V

P2 = n2RT/V

total pressure P = P1 + P2 = (n1+n2) *RT/V

The fraction of P due to the second gas is then

P2/P = (n2RT/V)/(n1+n2) *RT/V = n2/(n1+n2)

n1 = 3.7

n2 = 0.3

P2/P = 0.075

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