(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

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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

In all spontaneous processes,which of the following is true?

For the reaction occurring in the gaseous phase: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,which of the following conditions is correct for the reaction to be spontaneous at high temperatures?

In which of the following conditions will a reaction always be spontaneous at all temperatures?

$\Delta G$ in the process of melting of ice at $-15\,^{\circ}C$ is

Calculate the amount of work done during isothermal expansion of a gas from a volume of $4 \ dm^{3}$ to $6 \ dm^{3}$ against a constant external pressure of $3 \ atm$ (in $J$)?

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