Use the following data: One mole each of A_2( g ) and B_2( g ) are taken in a 1 L closed flask and allowed to establish the equilibrium at 500K. A_2(…

Use the following data :

Substance	$\displaystyle \frac{\Delta_f \mathrm{H}^{\ominus}(500 \mathrm{~K})}{\mathrm{kJ} \mathrm{mol}^{-1}}$	$\displaystyle \frac{\mathrm{S}^{\ominus}(500 \mathrm{~K})}{\mathrm{JK}^{-1} \mathrm{~mol}^{-1}}$
AB(g)	$\displaystyle 32$	$\displaystyle 222$
$\displaystyle \mathrm{A}_2(\mathrm{~g})$	$\displaystyle 6$	$\displaystyle 146$
$\displaystyle \mathrm{B}_2(\mathrm{~g})$	$\displaystyle x$	$\displaystyle 280$

One mole each of $\displaystyle \mathrm{A}_2(\mathrm{~g})$ and $\displaystyle \mathrm{B}_2(\mathrm{~g})$ are taken in a $\displaystyle 1$ L closed flask and allowed to establish the equilibrium at 500K. $$\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{~g}) $$ The value of $\displaystyle x$ (in $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$ ) is $\displaystyle \_\_\_\_$. (Nearest integer) (Given : $\displaystyle \log \mathrm{K}=2.2 \quad \mathrm{R}=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ )