1. Tardigrade
  2. Question
  3. Chemistry
  4. For the reaction CO(g)+(1/2)O2(g) xrightarrow[] CO2(g),Δ H and Δ S are -283kJ and -87JK-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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Q. For the reaction $ CO(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow[{}]{{}} $ $ C{{O}_{2}}(g),\Delta H $ and $ \Delta S $ are $ -283kJ $ and $ -87J{{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?

KEAMKEAM 2006

Solution:

$ \because $ $ \Delta G=\Delta H-T.\Delta S $ For a spontaneous reaction $ \Delta G $ should be negative $ \Delta H=-238\text{ }kJ,\Delta S=-\text{ }87\text{ }J{{K}^{-1}} $ Hence, reaction will be spontaneous when $ \Delta H>T.\Delta S $ . Therefore, at 1000, 1500 and 3000 K the reaction would be spontaneous.