(B) The spontaneity of a reaction is determined by the Gibbs free energy change $(\Delta G)$,given by the equation: $\Delta G = \Delta H - T\Delta S$.

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(B) The spontaneity of a reaction is determined by the Gibbs free energy change $(\Delta G)$,given by the equation: $\Delta G = \Delta H - T\Delta S$. Given: $\Delta H = -11.7 \times 10^3 \, J \, mol^{-1}$,$\Delta S = -105 \, J \, mol^{-1} K^{-1}$,and $T = 25 + 273 = 298 \, K$. Substituting the values: $\Delta G = (-11.7 \times 10^3) - (298 \times -105)$. $\Delta G = -11700 + 31290 = +19590 \, J \, mol^{-1}$. Since $\Delta G > 0$,the reaction is non-spontaneous.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:

A
Spontaneous
B
Non-spontaneous
C
At equilibrium
D
Cannot be determined

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The $\Delta G$ in the process of melting of ice at $-15\,^{\circ}C$ is

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When $\Delta H_{vap} = 30 \ kJ \ mol^{-1}$ and $\Delta S_{vap} = 75 \ J \ mol^{-1} \ K^{-1}$,then the temperature of vapour,at one atmosphere is . . . . $K$.

MediumJEE MAIN 2024

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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 $.99$)

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One mole of an ideal gas at $1 \ atm$ pressure is filled in a bulb of $10 \ L$ capacity and is connected to a vacuum bulb of $100 \ L$ capacity. How much work is done in this process in Joules?

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The reaction $MgO_{(s)} + C_{(s)} \to Mg_{(s)} + CO_{(g)}$,for which $\Delta_r H^o = +491.1 \ kJ \ mol^{-1}$ and $\Delta_r S^o = 198.0 \ J \ K^{-1} \ mol^{-1}$,is not feasible at $298 \ K$. The temperature above which the reaction will be feasible is ..... $K$.

DifficultJEE MAIN 2019

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For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:

Similar Questions

The $\Delta G$ in the process of melting of ice at $-15\,^{\circ}C$ is

When $\Delta H_{vap} = 30 \ kJ \ mol^{-1}$ and $\Delta S_{vap} = 75 \ J \ mol^{-1} \ K^{-1}$,then the temperature of vapour,at one atmosphere is . . . . $K$.

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

One mole of an ideal gas at $1 \ atm$ pressure is filled in a bulb of $10 \ L$ capacity and is connected to a vacuum bulb of $100 \ L$ capacity. How much work is done in this process in Joules?

The reaction $MgO_{(s)} + C_{(s)} \to Mg_{(s)} + CO_{(g)}$,for which $\Delta_r H^o = +491.1 \ kJ \ mol^{-1}$ and $\Delta_r S^o = 198.0 \ J \ K^{-1} \ mol^{-1}$,is not feasible at $298 \ K$. The temperature above which the reaction will be feasible is ..... $K$.

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