Question

A vessel with a volume of 41.8 L contains 2.80 g of nitrogen gas, 0.403 g of hydrogen gas, and 79.9 g of argon gas. At 25°C, what is the pressure in the vessel?

A)1.52 B)56.2 atm C)1.35 atm D)48.6 atm E)0.113 atm

thanks in advance please explain as thoroughly as possible

Answer 1

Molar mass of N₂ = 28 g/mole

Molar mass of H₂ = 2 g/mole

Molar mass of Ar = 40 g/mole

Thus, moles of N₂ in 2.8 g of it = mass/molar mass = 2.8/28 = 0.1

moles of H₂ in 0.403 g of it = mass/molar mass = 0.403/2 = 0.202

moles of Ar in 79.9 g of it = mass/molar mass = 79.9/40 = 1.998

Total moles of the gases = 0.1+0.202+1.998 = 2.3

Applying Ideal gas equation we get,

Pressure of the gas mixture,P = (n*R*T)/V = (2.3*0.0821*298)/41.8 = 1.346 atm

Thus, the correct option is :- (C)