(C) The relationship for Gibbs energy is given by $\Delta G = \Delta H - T\Delta S$. For $\Delta G = 0$,the equation becomes $\Delta H = T\Delta S$. G

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(C) The relationship for Gibbs energy is given by $\Delta G = \Delta H - T\Delta S$. For $\Delta G = 0$,the equation becomes $\Delta H = T\Delta S$. Given $\Delta H = 40.63 \ kJ/mol = 40630 \ J/mol$ and $\Delta S = 108.8 \ J/K \cdot mol$. Substituting the values: $T = \frac{\Delta H}{\Delta S} = \frac{40630 \ J/mol}{108.8 \ J/K \cdot mol} = 373.4 \ K$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

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 $.4$)?

A
$273$
B
$393$
C
$373$
D
$293$

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Thermodynamics

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Free energy and Work

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 :

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The dependence of Gibbs free energy on pressure for an isothermal process of an ideal gas is given by:

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For a spontaneous process,which of the following conditions must be met?

Easy

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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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$A$ process has $\Delta H = 200 \ J \ mol^{-1}$ and $\Delta S = 40 \ J \ K^{-1} \ mol^{-1}$. Choose the minimum temperature above which the process will be spontaneous.

MediumJEE MAIN 2019

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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 $.4$)?

Similar Questions

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 :

The dependence of Gibbs free energy on pressure for an isothermal process of an ideal gas is given by:

For a spontaneous process,which of the following conditions must be met?

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 $kJ \ mol^{-1}$?

$A$ process has $\Delta H = 200 \ J \ mol^{-1}$ and $\Delta S = 40 \ J \ K^{-1} \ mol^{-1}$. Choose the minimum temperature above which the process will be spontaneous.

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