(B) At equilibrium,the Gibbs free energy change $\Delta G$ is equal to $0$.Using the relation $\Delta G = \Delta H - T \Delta S = 0$,we get $T = \frac

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(B) At equilibrium,the Gibbs free energy change $\Delta G$ is equal to $0$.Using the relation $\Delta G = \Delta H - T \Delta S = 0$,we get $T = \frac{\Delta H}{\Delta S}$.Given $\Delta H = -165 \ kJ \ mol^{-1} = -165000 \ J \ mol^{-1}$ and $\Delta S = -550 \ J K^{-1} mol^{-1}$.Substituting the values: $T = \frac{-165000 \ J \ mol^{-1}}{-550 \ J K^{-1} mol^{-1}} = 300 \ K$.Therefore,the temperature at which the reaction attains equilibrium is $300 \ K$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

The standard entropy change for the reaction $4 Fe ( s ) + 3 O_{2} ( g ) \rightarrow 2 Fe_{2} O_{3} ( s )$ is $-550 \ J K^{-1}$ at $298 \ K$. Given: The standard enthalpy change for the reaction is $-165 \ kJ \ mol^{-1}$. The temperature in $K$ at which the reaction attains equilibrium is ... . (Nearest Integer)

JEE MAIN 2022 All JEE MAIN

A
$30$
B
$300$
C
$210$
D
$670$

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If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?

EasyAP EAMCET 2023

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For a reaction $\Delta H = -30 \ kJ$ and $\Delta S = -45 \ J \ K^{-1}$,at what temperature does the reaction change from spontaneous to non-spontaneous (in $K$)?

EasyMHT CET 2020

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For the melting of $3 \ moles$ of water at $0 \, ^\circ C$,the $\Delta G^o$ is:

Easy

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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 is correct?

Medium

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If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?

For a reaction $\Delta H = -30 \ kJ$ and $\Delta S = -45 \ J \ K^{-1}$,at what temperature does the reaction change from spontaneous to non-spontaneous (in $K$)?

For the melting of $3 \ moles$ of water at $0 \, ^\circ C$,the $\Delta G^o$ 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 is correct?

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