Question

The value of $log_{10}K$ for a reaction A ⇋ B is

(Given,

$\Delta H^{\circ}_{298K}$ = –54.67 kJ $mol^{-1}$

$\Delta H^{\circ}_{298K}$ = 10 kJ $mol^{-1}$

and R = 8.314 J $K^{-1}mol^{-1}$

2.303 × 8.314 × 298 = 5705)

Answer 1

$\Delta G^{\circ}$ = $\Delta H^{\circ}-T\Delta S^{\circ}$

= –54.07 × 1000 – 298 × 10

= –57050 ΔGº

= –2.303 RT$log_{10}$K

logK = 10