(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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Free energy and Work

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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 $27 \ ^oC$?

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The enthalpy and entropy change for the reaction $Br_{2(l)} + Cl_{2(g)} \rightarrow 2BrCl_{(g)}$ are $30 \ kJ \ mol^{-1}$ and $105 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature at which the reaction will be in equilibrium is ............... $K$.

For a reaction to be spontaneous at any temperature,which of the following is true?

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

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