Question 75. For a certain thermochemical reaction M \rightarrow N at
T=400 ~K, \Delta H^{\ominus}=77.2 ~kJ ~mol^{-1}, \Delta ~S=122 ~JK^{-1},
\log equilibrium constant (\log K) is – \times 10^{-1}.
Answer (37)
Explanation:
\Delta G^{\circ}=\Delta H^{\circ}-T \Delta S^{\circ} =77.2 \times 10^{3}-400 \times 122=28400 ~J \Delta G^{\circ}=-2.303 RT \log K \Rightarrow 28400=-2.303 \times 8.314 \times 400 \log K \Rightarrow \log K=-3.708=-37.08 \times 10^{-1}