For a reaction M2O(s)→2M(s)+12O2(g); ΔH=30 kJ mol−1 and ΔS=0.07 – InterviewSolution

1.	For a reaction M2O(s)→2M(s)+12O2(g); ΔH=30 kJ mol−1 and ΔS=0.07 kJ K−1 mol−1 at 1 atm. Calculate minimum temperature (in K) at which the reaction would become spontaneous.
Answer» For a reaction $M_{2} O (s) \to 2 M (s) + \frac{1}{2} O_{2} (g); Δ H = 30 k J m o l^{- 1} a n d Δ S = 0.07 k J K^{- 1} m o l^{- 1} a t 1 a t m .$ Calculate minimum temperature (in $K$ ) at which the reaction would become spontaneous.

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