(B) For a reaction to occur reversibly,the change in Gibbs free energy must be zero,i.e.,$\Delta G = 0$. Using the relation $\Delta G = \Delta H - T\D

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(B) For a reaction to occur reversibly,the change in Gibbs free energy must be zero,i.e.,$\Delta G = 0$. Using the relation $\Delta G = \Delta H - T\Delta S$,we set $\Delta H - T\Delta S = 0$. Given $\Delta H_r = 100\, kJ/mol = 100,000\, J/mol$ and $\Delta S_r = 400\, J/mol\cdot K$. Substituting the values: $100,000 - T(400) = 0$. $T = \frac{100,000}{400} = 250\, K$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

For the given reaction: $H_{2(g)} + S_{(s)} \to H_2S_{(g)}$; $\Delta H_r = 100\, kJ/mol$ and $\Delta S_r = 400\, J/mol\cdot K$. The temperature at which the above reaction occurs reversibly is (Assuming $\Delta H_r$ and $\Delta S_r$ are independent of temperature) ..... $K$.

A
$200$
B
$250$
C
$400$
D
None

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Thermodynamics

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Free energy and Work

For a spontaneous change,free energy change $\Delta G$ is

Easy

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For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

MediumAIPMT 2010

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Gibbs free energy $G$,enthalpy $H$ and entropy $S$ are interrelated as in

Easy

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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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For the reaction $H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}$,$\Delta H = -285.8 \ kJ \ mol^{-1}$,$\Delta S = -0.163 \ kJ \ mol^{-1} K^{-1}$. What is the value of free energy change at $27 \ ^\circ C$ for the reaction in $kJ \ mol^{-1}$?

Medium

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For the given reaction: $H_{2(g)} + S_{(s)} \to H_2S_{(g)}$; $\Delta H_r = 100\, kJ/mol$ and $\Delta S_r = 400\, J/mol\cdot K$. The temperature at which the above reaction occurs reversibly is (Assuming $\Delta H_r$ and $\Delta S_r$ are independent of temperature) ..... $K$.

Similar Questions

For a spontaneous change,free energy change $\Delta G$ is

For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

Gibbs free energy $G$,enthalpy $H$ and entropy $S$ are interrelated as in

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 $...... \ K$.

For the reaction $H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}$,$\Delta H = -285.8 \ kJ \ mol^{-1}$,$\Delta S = -0.163 \ kJ \ mol^{-1} K^{-1}$. What is the value of free energy change at $27 \ ^\circ C$ for the reaction in $kJ \ mol^{-1}$?

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