Question

Q1. A gaseous mixture contains 10gram of H2. 196g of nitrogen 192 gram of
oxygen. Pressure of hydrogen is 1.9atm. calculate the partial pressure of oxygen

gas and nitrogen gas.

Answer 1

$P=n($ $RT\over V$ $)$ $-n_{constant}$

Moles of $N_2=n_{n_2}$ $=196g\over 28g/mol$ $=7mol$

Moles of $O_2=n_{O_2}=$ $192g\over 32g/mol$ $=6mol$

From the ideal gas law;

$P_{N_2}=$ $n_{N_2}RT\over V$

$=$ ${7mol\times 0.08206{atm.L\over mol.K} \times 273K}\over1L$ $=156.82atm$

$P_{O_2}=$ ${6mol\times 0.08206{atm.L\over mol.K} \times 273K}\over 1L$ $=134.0atm$

The partial pressure of $N_2$ $=156.82atm$

The partial pressure of$O_2=134atm$