Question

1 mole of $N_2{O}_4\left(g\right)$ at 300K is kept in a closed container under 1 atm pressure. It is heated to 600K 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. 2.0 atm
• D. 1.0 atm

Answer 1

The correct option is B 2.4 atm

Correct option is b).
$\begin{array}{cccc}& N_2{O}_4\leftrightharpoons & 2N{O}_2& \\ Initialmoles& 1& 0& \end{array}$

Total moles=0.8+0.4=1.2

Applying, $PV=nRT$, at constant volume,

$\frac{P1}{n1T1}=\frac{P}{n2T2}$

$\frac{1}{1X300}=\frac{P_2}{1.2X600}$

$P_2=2.4atm.$