(A) Given: $\Delta H = 40.63 \ kJ \ mol^{-1} = 40630 \ J \ mol^{-1}$ $\Delta S = 100 \ J \ K^{-1} \ mol^{-1}$ $T = 27 \ ^oC = 27 + 273 = 300 \ K$ The

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(A) Given: $\Delta H = 40.63 \ kJ \ mol^{-1} = 40630 \ J \ mol^{-1}$ $\Delta S = 100 \ J \ K^{-1} \ mol^{-1}$ $T = 27 \ ^oC = 27 + 273 = 300 \ K$ The Gibbs free energy equation is $\Delta G = \Delta H - T \Delta S$. Substituting the values: $\Delta G = 40630 - (300 \times 100)$ $\Delta G = 40630 - 30000 = 10630 \ J \ mol^{-1}$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

For a certain reaction,the enthalpy change and entropy change are $40.63 \ kJ \ mol^{-1}$ and $100 \ J \ K^{-1} \ mol^{-1}$ respectively. What will be the value of $\Delta G$ at $27 \ ^oC$?

A
$10630 \ J \ mol^{-1}$
B
$10789 \ J \ mol^{-1}$
C
$11532 \ J \ mol^{-1}$
D
$10576 \ J \ mol^{-1}$

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Thermodynamics

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Free energy and Work

For a reaction at $25^o C$,$\Delta H > 0$ and $\Delta S > 0$. Under what conditions will this reaction become spontaneous?

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The standard enthalpy for the decomposition of $N_2O_5$ to $NO_2$ is $58.04 \ kJ$ and standard entropy of this reaction is $176.7 \ J/K$. The standard free energy change for this reaction at $25 \ ^oC$ is .................. $kJ$.

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Which of the following conditions will always lead to a non-spontaneous change?

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For the change $H_2O_{(l)} \to H_2O_{(g)}$ at $P = 1 \ atm$ and $T = 373 \ K$,the free energy change $\Delta G = 0$. This indicates that:

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For a certain reaction,the enthalpy change and entropy change are $40.63 \ kJ \ mol^{-1}$ and $100 \ J \ K^{-1} \ mol^{-1}$ respectively. What will be the value of $\Delta G$ at $27 \ ^oC$?

Similar Questions

For a reaction at $25^o C$,$\Delta H > 0$ and $\Delta S > 0$. Under what conditions will this reaction become spontaneous?

$A$ $4.50 \ g$ sample of methane occupies $12.7 \ L$ at $310 \ K$. Calculate the work done in $J$ when the gas undergoes isothermal expansion against a constant external pressure of $200 \ torr$ until the volume increases by $3.3 \ L$. (in $.99$)

The standard enthalpy for the decomposition of $N_2O_5$ to $NO_2$ is $58.04 \ kJ$ and standard entropy of this reaction is $176.7 \ J/K$. The standard free energy change for this reaction at $25 \ ^oC$ is .................. $kJ$.

Which of the following conditions will always lead to a non-spontaneous change?

For the change $H_2O_{(l)} \to H_2O_{(g)}$ at $P = 1 \ atm$ and $T = 373 \ K$,the free energy change $\Delta G = 0$. This indicates that:

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