Question

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?

Answer 1

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"`?