Question

Calculate the total pressure in a 10.0 liter flask at 27°C of a sample of gas that contains 6.0 grams of hydrogen, 15.2 grams of nitrogen, and 16.8 grams of helium.

Answer 1

The total pressure is 27.8 atm

Step-by-step explanation:

From the ideal gas equation,

PV = nRT

P (total pressure) = nRT/V

n (total moles of gases) = (6/1 moles of hydrogen) + (15.2/14 moles of nitrogen) + (16.8/4 moles of helium) = 6+1.1+4.2 = 11.3 moles

R = 0.082057L.atm/gmol.K, T = 27°C = 27+273K = 300K, V = 10L

P = 11.3×0.082057×300/10 = 27.8 atm