(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

What is the nature of the reaction at $298 \ K$,if the entropy change and enthalpy change for a chemical reaction are $7.4 \ cal \ K^{-1}$ and $-2.5 \times 10^3 \ cal$,respectively?

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For a reaction $\Delta H = 9.08 \ kJ \ mol^{-1}$ and $\Delta S = 35.7 \ J \ K^{-1} \ mol^{-1}$. Which of the following statements is correct for the reaction?

Medium

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For the melting of $3 \ mol$ of ice at $0^o \text{C}$,$\Delta G = \dots \dots$

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$A$ process is taking place at constant temperature and pressure. Then

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Calculate the value of $\Delta G$ for the following reaction: $N_2O_{4(g)} \longrightarrow 2NO_{2(g)}$ if $\Delta H = 57.44 \ kJ$ and $\Delta S = 176 \ J \ K^{-1} \ mol^{-1}$ at $300 \ K$. (in $kJ$)

MediumMHT CET 2024

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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

What is the nature of the reaction at $298 \ K$,if the entropy change and enthalpy change for a chemical reaction are $7.4 \ cal \ K^{-1}$ and $-2.5 \times 10^3 \ cal$,respectively?

For a reaction $\Delta H = 9.08 \ kJ \ mol^{-1}$ and $\Delta S = 35.7 \ J \ K^{-1} \ mol^{-1}$. Which of the following statements is correct for the reaction?

For the melting of $3 \ mol$ of ice at $0^o \text{C}$,$\Delta G = \dots \dots$

$A$ process is taking place at constant temperature and pressure. Then

Calculate the value of $\Delta G$ for the following reaction: $N_2O_{4(g)} \longrightarrow 2NO_{2(g)}$ if $\Delta H = 57.44 \ kJ$ and $\Delta S = 176 \ J \ K^{-1} \ mol^{-1}$ at $300 \ K$. (in $kJ$)

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