Problem: A gas mixture with a total pressure of 760 mmHg contains each of the following gases at the indicated partial pressures: 126 mmHg CO2, 220 mmHg Ar, and 188 mmHg O2. The mixture also contains helium gas.What mass of helium gas is present in a 12.6-L sample of this mixture at 274 K ?

FREE Expert Solution

Calculate the pressure of helium gas:

Ptotal=PCO2+PAr+PO2+PHePHe=Ptotal-(PCO2+PAr+PO2)PHe=760 mmHg-(126 mmHg+220 mmHg+188 mmHg)

PHe = 226 mmHg


Calculate the pressure in atm:

1 atm = 760 mmHg

PHe=226 mmHg×1 atm760 mmHg

PHe = 0.2974 atm


Ideal Gas Law:

PV=nRT

moles (n)=mass (m)molar mass (M)

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Problem Details

A gas mixture with a total pressure of 760 mmHg contains each of the following gases at the indicated partial pressures: 126 mmHg CO2, 220 mmHg Ar, and 188 mmHg O2. The mixture also contains helium gas.

What mass of helium gas is present in a 12.6-L sample of this mixture at 274 K ?

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