Question

A. What is the mole fraction of each component in a mixture of 12.63 g of H2, 66.89 g of N2, and 19.55 g of NH3?

Express your answers using three significant figures separated by commas.

B. A special gas mixture used in bacterial growth chambers contains 1.00 % by weight CO2 and 99.0 % O2.

What is the partial pressure (in atmospheres) of each gas at a total pressure of 0.871 atm ?

Enter your answers numerically separated by a comma.

Answer 1

a)

mol of H2 = mass/MW = 12.63/2 = 6.315

mol of N2 mass/MW = 66.89/28 = 2.3889

mol of NH3 = mass/MW = 19.55/17 = 1.15

total mol = 6.315+2.3889+1.15 = 9.8539

x-H2 = mol of H2 / Total mol = 6.315/9.8539 = 0.640

x-N2= mol of N2/ Total mol = 2.3889/9.8539 = 0.242

x-NH3 = mol of NH3 / Total mol = 1.15/9.8539 = 0.117

B)

assume 100 g of mix

mas sof CO2 = 1

mass of O2 = 99

change to mol

mol fo CO2= mass/MW = 1/44 = 0.0227

mol of O2 = mass/MW = 99/32 = 3.094

P-O2 = 3.094/(3.094+0.0227) * 0.871 = 0.8646 atm

P-CO2= 0.0227/(3.094+0.0227) * 0.871 =0.00634 atm