A closed 5.00 L container is filled with a mixture of 4.00 moles of hydrogen gas, 8.00 moles of oxygen, 12.0 moles of helium, and 6.00 moles of nitrogen. What is the pressure due to the oxygen in this container at a temperature of 25 °C?

24.44 atm

Explanation:

Considering that this gas mixture behaves like an ideal gass, and that all component gases are ideal gases, we can use:

PV=nRT

Then:

P=nRT/V

Where:

n = N° of moles

R = gas constant = 0.082 Lt*atm/K*mol

T = temperature (in Kelvin)

V = volume (in Lt)

Finally, statement says:

T = 25°C = 298 K

V = 5 Lt

n = 8 moles (for O₂)

P = [8 molx (0.082 Lt*atm/K*mol) x298 K]/5 Lt

P = 24.44 atm would be the pressure due to O₂ (partial pressure of the oxygen)