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

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(C) The spontaneity of a reaction is determined by the Gibbs free energy change,given by the equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be spontaneous at all temperatures,$\Delta G$ must be negative $(\Delta G If $\Delta H 0$ (increase in entropy),then $\Delta G$ will always be negative regardless of the temperature $T$,because both terms ($\Delta H$ and $-T\Delta S$) will contribute to a negative value. Therefore,the correct condition is $\Delta H 0$.

Class 11 Chemistry Thermodynamics Free energy and Work

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Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous at all temperatures.

MHT CET 2025 All MHT CET

A
$\Delta H > 0$ and $\Delta S > 0$
B
$\Delta H < 0$ and $\Delta S < 0$
C
$\Delta H < 0$ and $\Delta S > 0$
D
$\Delta H > 0$ and $\Delta S < 0$

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For the vaporization of water at $1 \ atm$ pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ/mol$ and $108.8 \ J/K \cdot mol$ respectively. At what temperature $(K)$ will the change in Gibbs energy $(\Delta G)$ be zero (in $.4$)?

Medium

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For the spontaneity of a reaction,which statement is always true?

Medium

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For the reaction at $298 \ K$,$2 \ A^{+}B \rightarrow C$. $\Delta H = 400 \ kJ \ mol^{-1}$ and $\Delta S = 0.2 \ kJ \ mol^{-1} \ K^{-1}$. The reaction will become spontaneous above $...... \ K$.

MediumJEE MAIN 2024

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At the transition temperature $T$,$\Delta G^0 = 0$ and $\Delta G^0 = 105 - 35 \log T$,where $A$ and $B$ are two states of substance $X$. The transition temperature in $^\circ\text{C}$ when pressure is $1 \text{ atm}$ is . . . . . . .

DifficultJEE MAIN 2026

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State the criteria for a spontaneous process in terms of $\Delta G$ at constant pressure and temperature.

Easy

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Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous at all temperatures.

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For the vaporization of water at $1 \ atm$ pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ/mol$ and $108.8 \ J/K \cdot mol$ respectively. At what temperature $(K)$ will the change in Gibbs energy $(\Delta G)$ be zero (in $.4$)?

For the spontaneity of a reaction,which statement is always true?

For the reaction at $298 \ K$,$2 \ A^{+}B \rightarrow C$. $\Delta H = 400 \ kJ \ mol^{-1}$ and $\Delta S = 0.2 \ kJ \ mol^{-1} \ K^{-1}$. The reaction will become spontaneous above $...... \ K$.

At the transition temperature $T$,$\Delta G^0 = 0$ and $\Delta G^0 = 105 - 35 \log T$,where $A$ and $B$ are two states of substance $X$. The transition temperature in $^\circ\text{C}$ when pressure is $1 \text{ atm}$ is . . . . . . .

State the criteria for a spontaneous process in terms of $\Delta G$ at constant pressure and temperature.

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