(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$.For a reaction to be spontaneous

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(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$.For a reaction to be spontaneous,$\Delta G $1$. If $\Delta H > 0$ and $\Delta S $2$. If $\Delta H > 0$ and $\Delta S > 0$,then $\Delta G $3$. If $\Delta H $4$. If $\Delta H 0$,then $\Delta G$ is always negative,so the reaction is spontaneous at all temperatures ($D$ is correct).Thus,conditions $A, C,$ and $D$ are correct. However,based on the provided options,the combination $A$ and $C$ is the most appropriate match.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

The effect of temperature on the spontaneity of reactions is represented as follows:

Condition Details

$A$. $\Delta H: +, \Delta S: -$ $T$: any $T$,Spontaneity: Non-spontaneous

$B$. $\Delta H: +, \Delta S: +$ $T$: low $T$,Spontaneity: Non-spontaneous

$C$. $\Delta H: -, \Delta S: -$ $T$: low $T$,Spontaneity: Spontaneous

$D$. $\Delta H: -, \Delta S: +$ $T$: any $T$,Spontaneity: Spontaneous

Which of the above conditions are correctly matched?

Condition	Details
$A$. $\Delta H: +, \Delta S: -$	$T$: any $T$,Spontaneity: Non-spontaneous
$B$. $\Delta H: +, \Delta S: +$	$T$: low $T$,Spontaneity: Non-spontaneous
$C$. $\Delta H: -, \Delta S: -$	$T$: low $T$,Spontaneity: Spontaneous
$D$. $\Delta H: -, \Delta S: +$	$T$: any $T$,Spontaneity: Spontaneous

JEE MAIN 2025 All JEE MAIN

A
$B$ and $D$ only
B
$A$ and $D$ only
C
$B$ and $C$ only
D
$A$ and $C$ only

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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 . . . . . . .

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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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Which of the following relations is correct?

EasyTS EAMCET 2021

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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?

Medium

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For $2 \ mol$ of $He$ (ideal gas),find the work done in a process where it is heated from $200 \ K$ to $400 \ K$ such that the enthalpy of the gas varies as : $H = 10 \ V^2$ (in $R$)

Difficult

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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 . . . . . . .

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 $.4$)?

Which of the following relations is correct?

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?

For $2 \ mol$ of $He$ (ideal gas),find the work done in a process where it is heated from $200 \ K$ to $400 \ K$ such that the enthalpy of the gas varies as : $H = 10 \ V^2$ (in $R$)

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