What is the total pressure in a 6.00-L flask which contains 0.127 mol of #H_2# (g) and 0.288 mol of #N_2# (g) at 20.0°C?

1 Answer
Jun 14, 2016

Answer:

Approx. #1.7*atm#

Explanation:

The pressures are additive by Dalton's Law of Partial Pressures: the pressure exerted by a gas in a gaseous mixture is the same as the pressure it would exert if it alone occupied the container. I could calculate the individual partial pressures, or simply calculate the pressure based on the COMBINED molar quantities:

#P=(nRT)/V# #=#

#(0.415*cancel(mol)xx0.0821*cancel(L)*atm*cancel(K^-1)*cancel(mol^-1)xx293*cancelK]/(6.00*cancelL)#
#~=# #??*atm#

Given what I have said, can you calculate the partial pressures, #P_"dihydrogen"#, and #P_"dinitrogen"#?