Question

For the equilibrium :
$LiCl.3N{H}_3\left(s\right)\rightleftharpoons LiCl.N{H}_3\left(s\right)+2N{H}_3\left(g\right),Kp=9at{m}^{2}at{27}^{\circ }C$. A 4.92 litre vessel contains 0.1 mole of $LiCl.N{H}_3$. The number of moles of $N{H}_3$ should be added to the flask at this temperature to drive the back ward reaction for completion is $(0.2\times y)$. The value of ‘y’ is ___

Answer 1

$kp=p^2,p=3atm$
$PV=nRT$
$3\times 4.92=0.082\times 300\times n$
$n=0.6$
$LiCl.N{H}_3\left(s\right)+2N{H}_3\left(g\right)\rightleftharpoons LiCl.3N{H}_3$
$\begin{array}{cccc}Initialmoles& 0.1& a& 0\\ molesofequilibrium& 0& (a–0.2)& 0.1\end{array}$
Moles of $N{H}_3=(a–0.2)=0.6$
$a=0.8$