InterviewSolution
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InterviewSolution
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For the reaction `CO (g) + (1)/(2) O_(2) (g) rarr CO_(2) (g)` `Delta H` and `Delta S` are `283 kJ` and `-87 J K^(-1)`, respectively. It was intended to carry out this reaction at 1000,1500,3000, and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous?A. 3000 and 3500 KB. 1500 and 3000 KC. 1500 , 3000, and 3500 KD. 1000, 1500, and 3000 K |
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Answer» Correct Answer - D According to thermodynamics, `Delta G = Delta H - T Delta S` Since both `Delta H` and `Delta S` are negative, the reaction will be spontaneous at a temperature below equilibrium temperature so that the `Delta H` term prdominates. At equilibrium, `Delta G = 0`. Thus, `T = (Delta H)/(Delta S) = (- 283 xx 10^(3) J)/(- 87 xx 10 J K^(-1)) = 3252 K` This implies that the reaction will be spontaneous at any temperature below `3252 K`. |
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