For a certain thermochemical reaction M → N at T =400 K, Δ H^ =77.2 kJ mol^-1, Δ S =122 JK^-1, log equilibrium constant ( log K ) is - ____ × 10^-1.

For a certain thermochemical reaction $\displaystyle \mathrm{M} \rightarrow \mathrm{N}$ at $\displaystyle \mathrm{T}=400 \mathrm{~K}, \Delta \mathrm{H}^{\ominus}=77.2 \mathrm{~kJ} \mathrm{~mol}^{-1}, \Delta \mathrm{~S}=122 \mathrm{JK}^{-1}$, log equilibrium constant $\displaystyle (\log \mathrm{K})$ is - $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-1}$.