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Question
For the reaction CO(g)+12O2(g)→CO2(g),ΔH and ΔS are −283 kJ and −87 J K−1 mol−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?
For the reaction CO(g)+12O2(g)→CO2(g),ΔH and ΔS are −283 kJ and −87 J K−1 mol−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?
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Solution
The correct option is C 1000, 1500 and 3000 K
By using the equation,
ΔG=ΔH−TΔSAt 1000K, ΔG=−283−(−1000×0.087)=−196 kJ (spontaneous)At 1500 K, ΔG=−283−(−1500×0.087)=−152.5 kJ (spontaneous)At 3000 K , ΔG=−283−(−3000×0.0987)=−22 kJ (spontaneous)At 3500 K, ΔG=−283−(−3500×0.087)=+21.5 kJ (Non-spontaneous)
By using the equation,
ΔG=ΔH−TΔSAt 1000K, ΔG=−283−(−1000×0.087)=−196 kJ (spontaneous)At 1500 K, ΔG=−283−(−1500×0.087)=−152.5 kJ (spontaneous)At 3000 K , ΔG=−283−(−3000×0.0987)=−22 kJ (spontaneous)At 3500 K, ΔG=−283−(−3500×0.087)=+21.5 kJ (Non-spontaneous)
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