Question

One mole of $N_2{O}_4\left(g\right)$ at 300 K is kept in a closed container under 1 atmosphere. It is heated to 600 K when $20\%$ by mass of $N_2{O}_4\left(g\right)$ decomposes to $N{O}_2\left(g\right)$. The resultant pressure is:

• A. 1.2 atm
• B. 2.4 atm
• C. 2 atm
• D. 5 atm

Answer 1

The correct option is B 2.4 atm

$\underset{1}{N_2{O}_4}$ $\underset{-}{2N{0}_2}$
$\underset{0.8}{1-0.2}$ $\underset{0.4}{2\times 0.2}$
$\frac{P_1{v}_1}{n_1{T}_1}=\frac{P_2{v}_2}{n_2{T}_2}$
$[v_1=v_2]$
$\frac{\left(2\right)}{1\times \left(300\right)}=\frac{P_2}{1.2\times 600}$ $[n_2=0.8+0.4=1.2]$
$P_2=2.4atm$