The partial pressure of nitrogen in the flask is

Question

A mixture of hydrogen and nitrogen gases, in a 8.04 L flask at 40 °C, contains 0.289 grams of hydrogen and 12.3 grams of nitrogen. The partial pressure of nitrogen in the flask is ________ atm and the total pressure in the flask is ________atm

Answer 1

The total pressure = Partial pressure of H2  + Partial pressure of N2

 

The total pressure (P) can be calculated using ideal gas equation: PV = nRT,

 

P = nRT/V

 

n = mole of H₂ + mol N₂ 

 

Find the mol using the given masss and molar mass for H2 and N2

 

mole H2 = 0.289 g/2.02g/mol = 0.143 mol

 

mol N2  = 12.3 g/28.0 g/mol  =  0.439 mol

 

n = 0.143 + 0.439 = 0.582 mol

 

Thus P = nRT/V , n =0.582 mol, R = 0.0821 L.atm/mol K, T = 40 + 273 = 313 K, V = 0.04 L

 

plug in the values and you will get P in atm.

 

Partial pressure H2 = (mole fraction H2) x P

 

                        = [0.143/(0.143 + 0.439)] x P

 

                        =-------- atm

 

Partial pressure N2 = (mole fraction of N2) x P

 

I will let you to complete the calculation.