Let us consider an endothermic reaction which | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T \Delta S$.Given that the

Vedclass · Accepted Answer

Both $\Delta H$ and $\Delta S$ are $(+ve)$

Vedclass · Answer

(A) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T \Delta S$.Given that the reaction is endothermic,$\Delta H > 0$ (positive).At low temperature (freezing point of water,$273 \ K$),the reaction is non-spontaneous,meaning $\Delta G > 0$. This implies $\Delta H > T \Delta S$.At high temperature (boiling point of water,$373 \ K$),the reaction is spontaneous,meaning $\Delta G For $\Delta G$ to become negative as temperature $T$ increases,$\Delta S$ must be positive. Thus,both $\Delta H$ and $\Delta S$ are positive.

Let us consider an endothermic reaction which is non-spontaneous at the freezing point of water. However,the reaction is spontaneous at the boiling point of water. Choose the correct option.

Similar Questions

The temperature in $K$ at which $\Delta G = 0$, for a given reaction with $\Delta H = -20.5 \ kJ \ mol^{-1}$ and $\Delta S = -50.0 \ J \ K^{-1} \ mol^{-1}$ is:

For a reaction at $25^o C$,$\Delta H > 0$ and $\Delta S > 0$. Under what conditions will this reaction become spontaneous?

$A$ process is taking place at constant temperature and pressure. Then

For the reaction $Ag_2O_{(s)} \rightarrow 2Ag_{(s)} + 1/2 O_{2_{(g)}}$,the value of $\Delta H = 30.56 \, kJ \, mol^{-1}$ and $\Delta S = 66 \, J \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the change in free energy for the reaction be zero?

Which of the following conditions results in a spontaneous chemical reaction?

Vedclass Test Series

Exam Paper Generator

Online Exam Module