Question

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

Answer 1

Answer:

333.6 atm

Explanation:

The following data were obtained from the question:

Mole of O2 (nO2) = 3.96 moles

Mole of N2 (nN2) = 7.49 moles

Mole of CO2 (nCO2) = 1.19 moles

Total pressure = 563 mmHg

Partial pressure of N2 =..?

Next, we shall determine the total number of mole in the container.

This can be obtained as follow:

Mole of O2 (nO2) = 3.96 moles

Mole of N2 (nN2) = 7.49 moles

Mole of CO2 (nCO2) = 1.19 moles

Total mole =?

Total mole = nO2 + nN2 + nCO2

Total mole = 3.96 + 7.49 + 1.19

Total mole = 12.64 moles

Next, we shall determine the mole fraction of N2.

This can be obtained as follow:

Mole fraction = mole of substance/total mole

Mole of N2 (nN2) = 7.49 moles

Total mole = 12.64 moles

Mole fraction of N2 =?

Mole fraction of N2 = 7.49/12.64

Finally, we shall determine the partial pressure of N2.

This can be obtained as follow:

Mole fraction of N2 = 7.49/12.64

Total pressure = 563 mmHg

Partial pressure of N2 =..?

Partial pressure = mole fraction x total pressure

Partial pressure of N2 = 7.49/12.64 x 563

Partial pressure of N2 = 333.6 atm

The, the partial pressure of nitrogen, N2 is 333.6 atm