(C) The spontaneity of a process is determined by the Gibbs free energy change,given by the equation $\Delta G = \Delta H - T\Delta S$. For a process

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Positive $\Delta H$ and negative $\Delta S$

(C) The spontaneity of a process is determined by the Gibbs free energy change,given by the equation $\Delta G = \Delta H - T\Delta S$. For a process to be non-spontaneous,$\Delta G$ must be positive $(> 0)$. When $\Delta H > 0$ (endothermic) and $\Delta S Therefore,the condition $\Delta H > 0$ and $\Delta S < 0$ always leads to a non-spontaneous change.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

Which of the following conditions will always lead to a non-spontaneous change?

A
Positive $\Delta H$ and positive $\Delta S$
B
Negative $\Delta H$ and negative $\Delta S$
C
Positive $\Delta H$ and negative $\Delta S$
D
Negative $\Delta H$ and positive $\Delta S$

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Thermodynamics

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Free energy and Work

For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:

Medium

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For a chemical reaction,if $\Delta H = \Delta S > 0$,then $\Delta H = $ ................

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For a reaction,$4 M (s) + n O_2 (g) \rightarrow 2 M_2 O_n (s)$,the free energy change is plotted as a function of temperature. The temperature below which the oxide is stable could be inferred from the plot as the point at which :

MediumJEE MAIN 2020

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$A$ chemical reaction cannot occur at all if

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Which of the following conditions will oppose or prevent a reaction from occurring?

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Which of the following conditions will always lead to a non-spontaneous change?

Similar Questions

For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:

For a chemical reaction,if $\Delta H = \Delta S > 0$,then $\Delta H = $ ................

For a reaction,$4 M (s) + n O_2 (g) \rightarrow 2 M_2 O_n (s)$,the free energy change is plotted as a function of temperature. The temperature below which the oxide is stable could be inferred from the plot as the point at which :

$A$ chemical reaction cannot occur at all if

Which of the following conditions will oppose or prevent a reaction from occurring?

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