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${\text{2PQ}} \rightleftharpoons {{\text{P}}_2}{\text{ + }}{{\text{Q}}_2}\,;\,\,\,\,{{\text{K}}_1}{\text{ = 2}}{\text{.5 }} \times \,{\text{1}}{{\text{0}}^5}\,$
${\text{PQ + }}\frac{1}{2}{R_2} \rightleftharpoons PQR\,;\,\,\,\,{{\text{K}}_2}{\text{ = 5 }} \times \,{\text{1}}{{\text{0}}^{ - 3}}\,$
The value of equilibrium constant for reaction
$\frac{1}{2}{{\text{P}}_2}{\text{ + }}\frac{1}{2}{{\text{Q}}_2}{\text{ + }}\frac{1}{2}{R_2} \rightleftharpoons PQR\,$ is
$H _{2} F _{2( g )} \rightarrow H _{2( g )}+ F _{2( g )}$
$\Delta U =-59.6\,kJ\,mol ^{-1} \text { at } 27^{\circ}\,C$.
The enthalpy change for the above reaction is (-) $kJ mol ^{-1}$ [nearest integer] Given : $R =8.314\,JK ^{-1}\,mol ^{-1}$
Assertion $A:$ In equation $\Delta_r G =- nFE _{\text {cell }}$ value of $\Delta_r G$ depends on $n$.
Reasons $R$ : $E_{\text {cell }}$ is an intensive property and $\Delta_{ r } G$ is an extensive property.
In the light of the above statements, choose the correct answer from the options given below
