Answer:
333.86 mmHg.
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.
