Discussion Forum

For the given reaction,

$H_{2}(g)+Cl_{2}{}(g)\rightarrow 2H^{+}(aq)+2Cl^{-}(aq).$

 $\triangle G^{0}=-262.4kJ$ 

 The value of free energy of formation

( $\triangle G^{0}_{f}$ ) for the ion Cl^-1 (aq)  . therefore will be

Answer:

Explanation:

$(\triangle G^{0}) reaction =\triangle G^{0}_{f}$   (products ) - $\triangle G^{0}_{f}$ (reactants)

$\therefore$    $264.4=[2\triangle G^{0}_{f} (H^{+})+2 \triangle G^{0}_{f}(C^{1-})]$

or   $264.4=-[\triangle G^{0}_{f} (H_{2})+ \triangle G^{0}_{f}(Cl_{2})]$

 $=[0+2\triangle G^{0}_{f}  (Cl^{-})]+[0+0]$

 or   $-262.4=2\triangle G^{0}_{f}(Cl^{-})$

 or  $-\triangle G^{0}_{f}(Cl^{-})=-131.2 kJmol^{-1}$