Question

What is the partial pressure of nitrogen gas (N2) in a container that contains 3.96 mol of oxygen gas (O2) , 7.49 mol of nitrogen gas (N2), and 1.19 mol of carbon dioxide gas (CO2) when the total pressure is 563 mmHg?

Answer 1

333.86 mmHg.

Step-by-step explanation:

Data obtained from the question include the following:

Mole of O2 = 3.96 moles

Mole of N2 = 7.49 moles

Mole of CO2 = 1.19 moles

Total pressure = 563 mmHg.

Next, we shall determine the mole fraction of nitrogen, N2.

This can be obtained as follow:

Total mole = n O2 + n N2 + n CO2

Total mole = 3.96 + 7.49 + 1.19

Total mole = 12.64 moles

Mole fraction of N2 = n N2/Total mole

Mole fraction of N2 = 7.49/12.64

Mole fraction of N2 = 0.593 mole.

Finally, we shall determine the partial pressure of nitrogen, N2.

This can be obtained as follow:

Mole fraction of N2 = 0.593 mole.

Total pressure = 563 mmHg.

Partial pressure of N2 =..?

Partial pressure = mole fraction x total pressure

Partial pressure of N2 = 0.593 x 563

Partial pressure of N2 = 333.86 mmHg.

Therefore, the partial pressure of nitrogen, N2 is 333.86 mmHg.