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?

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.

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i