(C) The spontaneity of a reaction is determined by the Gibbs free energy change,$\Delta G = \Delta H - T\Delta S$. At equilibrium,$\Delta G = 0$,so $T

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(C) The spontaneity of a reaction is determined by the Gibbs free energy change,$\Delta G = \Delta H - T\Delta S$. At equilibrium,$\Delta G = 0$,so $T = \frac{\Delta H}{\Delta S}$. Given $\Delta H = -40,000 \, J$ and $\Delta S = -50 \, J/K$,the equilibrium temperature is $T = \frac{-40,000 \, J}{-50 \, J/K} = 800 \, K$. For $\Delta H 800 \, K$. Thus,the transition occurs around $800 \, K$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

For a reaction,$\Delta H = -40 \, kJ$ and $\Delta S = -50 \, J/K$. At what temperature range will it change from spontaneous to non-spontaneous?

A
$0.8 \, K$ to $1 \, K$
B
$799 \, K$ to $800 \, K$
C
$800 \, K$ to $801 \, K$
D
$799 \, K$ to $801 \, K$

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Thermodynamics

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Free energy and Work

At constant pressure and temperature,the direction of any spontaneous chemical reaction is towards the state where there is a decrease in

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For reaction $Ag_2O_{(s)} \to 2Ag_{(s)} + 1/2 O_{2(g)}$,the value of $\Delta H = 30.56 \ kJ \ mol^{-1}$ and $\Delta S = 0.066 \ kJ \ K^{-1} \ mol^{-1}$. Temperature at which free energy change for reaction will be zero,is ............. $K$.

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For a certain reaction,$\Delta H = -225 \ kJ \ mol^{-1}$ and $\Delta S = -150 \ J \ K^{-1} \ mol^{-1}$. Find the temperature at which $\Delta G$ is zero. (in $K$)

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The essential condition for the feasibility of a reaction is that

Medium

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In which of the following conditions can a chemical reaction not occur?

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For a reaction,$\Delta H = -40 \, kJ$ and $\Delta S = -50 \, J/K$. At what temperature range will it change from spontaneous to non-spontaneous?

Similar Questions

At constant pressure and temperature,the direction of any spontaneous chemical reaction is towards the state where there is a decrease in

For reaction $Ag_2O_{(s)} \to 2Ag_{(s)} + 1/2 O_{2(g)}$,the value of $\Delta H = 30.56 \ kJ \ mol^{-1}$ and $\Delta S = 0.066 \ kJ \ K^{-1} \ mol^{-1}$. Temperature at which free energy change for reaction will be zero,is ............. $K$.

For a certain reaction,$\Delta H = -225 \ kJ \ mol^{-1}$ and $\Delta S = -150 \ J \ K^{-1} \ mol^{-1}$. Find the temperature at which $\Delta G$ is zero. (in $K$)

The essential condition for the feasibility of a reaction is that

In which of the following conditions can a chemical reaction not occur?

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