Partial pressures of gases?
A mixture of 1.00 g of H2(g) and 1.00 g of He(g) is placed in a 1.00 L flask at 27.0 degrees C. What are the partial pressures of each gas?
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A mixture of 1.00 g of H2(g) and 1.00 g of He(g) is placed in a 1.00 L flask at 27.0 degrees C. What are the partial pressures of each gas?
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Verified answer
Use PV = nRT for each gas.
P is what you are looking for;
V = 1 L
R is the universal gas constant (8.314)
T is temperature in Kelvin (27+273)
n is the number of moles of each gas (mass of gas divided by molar mass)
p of H2 = 1g/2 (.0821) (300)/(1) = 12.3
p of He = 1g/4 (.o821) (300)/(1) = 6.16