Question:medium

The entropy and enthalpy changes for the reaction \( \text{CO(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \) at 300 K and 1 atm are respectively \(-42.4 \text{ JK}^{-1}\) and \(-41.2 \text{ kJ}\). The temperature at which the reaction will go in the reverse direction is

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The sign of \(\Delta G\) determines the direction of a reaction. The equilibrium temperature \(T_{eq} = \Delta H / \Delta S\) is the "tipping point". If \(\Delta H\) and \(\Delta S\) have the same sign, the spontaneity depends on temperature. - If both are negative (as here), the reaction is spontaneous at low T (\(<T_{eq}\)) and non-spontaneous at high T (\(>T_{eq}\)). - If both are positive, the reverse is true.

Updated On: Mar 30, 2026

761.8 K
671.8 K
961.8 K
971.8 K

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The Correct Option is D

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