Chemical Thermodynamics Question 401

Question: For the reaction $ CO(g)+\frac{1}{2}O_2(g)\xrightarrow{{}}CO_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-

Options:

A) 1500 and 3500 K

B) 3000 and 3500 K

C) 1000, 1500 and 3000 K

D) 1500, 3000 and 3500 K

Show Answer

Answer:

Correct Answer: C

Solution:

$ \therefore \Delta G=\Delta H-T\times \Delta S $ For a spontaneous reaction, $ \Delta G $ should be negative $ \Delta H=-238kJ,\Delta S=-87J{{K}^{-1}} $

Hence, reaction will be spontaneous when $ \Delta H>T\times \Delta S $ . Therefore, at 1000, 1500 and 3000 K the reaction would be spontaneous.



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