Assuming ideal behaviour, the magnitude of log K for the following reaction at 25°C is x * 10^-1. The value of x is ………………… (integer answer)

3HC  $\equiv C{H}_{\left(g\right)}?C_6{H}_{6\left(I\right)}$

[Given : ${\Delta }_{f}G°\left(HC\equiv CH\right)$  = -2.04 * 10⁵J mol^-1 ; ${\Delta }_{f}G°\left(C_6{H}_6\right)=-1.24*10^{5}Jmo{l}^{-1}:$ R = 8.314 JK^-1mol^-1]

$3CH\equiv CH\left(g\right)\to C_6{H}_6\left(\mathcal{l}\right)$       

$\Delta G^0=-RT\mathcal{l}nK.........\left(i\right)$

$\Delta G^0=\sum \Delta {G^0}_P-\sum \Delta {G^0}_R..........\left(ii\right)$    

Equating (i) & (ii)

-2.303 RTlogk = 4.88 * 10⁵

$logK=\frac{-4.88*10^5}{2.303*R*T}=\frac{-488000}{5705.848}=-85.52=-855*10^{-1}$

So; magnitude of log K = 855 * 10^-1