(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G = \Delta H - T\Delta S$ must be negative $(\Delta G 0

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$\Delta H > 0$ and $\Delta S < 0$

(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G = \Delta H - T\Delta S$ must be negative $(\Delta G If $\Delta H > 0$ (endothermic) and $\Delta S Since both terms are positive,$\Delta G$ will always be positive regardless of the temperature $T$.Therefore,the reaction is non-spontaneous under all conditions.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

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

A
$\Delta H > 0$ and $\Delta S > 0$ with $T\Delta S > \Delta H$
B
$\Delta H < 0$ and $\Delta S < 0$ with $\Delta H > T\Delta S$
C
$\Delta H > 0$ and $\Delta S < 0$
D
$\Delta H < 0$ and $\Delta S > 0$

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Class 11

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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?

EasyAP EAMCET 2019

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For the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $373 \ K$ and $1 \ atm$ pressure,which of the following is true?

Medium

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What is the value of $\Delta G$ for a water system in an environment at a temperature of $100 \ K$?

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For the reaction $x + y \rightarrow z$,the process is spontaneous at room temperature,and the reverse reaction is spontaneous at high temperature. Which of the following is true?

Medium

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$A$ $4.50 \ g$ 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 $.99$)

Medium

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

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 the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $373 \ K$ and $1 \ atm$ pressure,which of the following is true?

What is the value of $\Delta G$ for a water system in an environment at a temperature of $100 \ K$?

For the reaction $x + y \rightarrow z$,the process is spontaneous at room temperature,and the reverse reaction is spontaneous at high temperature. Which of the following is true?

$A$ $4.50 \ g$ 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 $.99$)

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