(D) The Gibbs free energy change is given by the equation: $\Delta G = \Delta H - T\Delta S$. For the reaction to be at equilibrium,$\Delta G = 0$. Su

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$463 \ \text{K}$,non-spontaneous

(D) The Gibbs free energy change is given by the equation: $\Delta G = \Delta H - T\Delta S$. For the reaction to be at equilibrium,$\Delta G = 0$. Substituting the given values: $0 = 30.558 \ \text{kJ} - T \times 0.066 \ \text{kJ K}^{-1}$. Solving for $T$: $T = \frac{30.558}{0.066} = 463 \ \text{K}$. Since $\Delta H > 0$ and $\Delta S > 0$,the reaction is endothermic and entropy-driven. For temperatures $T 0$. Therefore,the reaction is non-spontaneous below $463 \ \text{K}$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

The $\Delta H$ and $\Delta S$ for a reaction at $1 \ \text{atm}$ pressure are $+30.558 \ \text{kJ}$ and $0.066 \ \text{kJ K}^{-1}$ respectively. The temperature at which the free energy change will be zero and below this temperature the nature of the reaction would be:

A
$483 \ \text{K}$,spontaneous
B
$443 \ \text{K}$,non-spontaneous
C
$443 \ \text{K}$,spontaneous
D
$463 \ \text{K}$,non-spontaneous

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$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?

Medium

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Enthalpy of hydrogenation of one mole of benzene to cyclohexane is
$[$Resonance energy of benzene $= -150.4 \ kJ / mol$.
Enthalpy of hydrogenation of cyclohexene $= -119.5 \ kJ / mol$ $]$

MediumTS EAMCET 2021

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If $\Delta G$ and $\Delta S$ for the reaction $A_{(g)} \rightarrow B_{(g)} + 2C_{(g)}$ at $2000 \ K$ are $-40 \ kJ \ mol^{-1}$ and $0.22 \ kJ \ K^{-1} \ mol^{-1}$ respectively,the change in internal energy for the same reaction approximately (in $kJ \ mol^{-1}$) is

MediumAP EAMCET 2023

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$\Delta H^o_f$ of water is $-285.5 \, kJ \, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3 \, kJ \, mol^{-1}$,$\Delta H^o_f$ of $OH^{-}$ ion will be.....$kJ \, mol^{-1}$

Medium

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An electric heater of power $600 \, W$ takes $8 \, \text{minutes}$ to evaporate $80 \, mL$ of water. The enthalpy of vaporization of water is ......... $kJ \, mol^{-1}$.

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The $\Delta H$ and $\Delta S$ for a reaction at $1 \ \text{atm}$ pressure are $+30.558 \ \text{kJ}$ and $0.066 \ \text{kJ K}^{-1}$ respectively. The temperature at which the free energy change will be zero and below this temperature the nature of the reaction would be:

Similar Questions

$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?

Enthalpy of hydrogenation of one mole of benzene to cyclohexane is$[$Resonance energy of benzene $= -150.4 \ kJ / mol$.Enthalpy of hydrogenation of cyclohexene $= -119.5 \ kJ / mol$ $]$

If $\Delta G$ and $\Delta S$ for the reaction $A_{(g)} \rightarrow B_{(g)} + 2C_{(g)}$ at $2000 \ K$ are $-40 \ kJ \ mol^{-1}$ and $0.22 \ kJ \ K^{-1} \ mol^{-1}$ respectively,the change in internal energy for the same reaction approximately (in $kJ \ mol^{-1}$) is

$\Delta H^o_f$ of water is $-285.5 \, kJ \, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3 \, kJ \, mol^{-1}$,$\Delta H^o_f$ of $OH^{-}$ ion will be.....$kJ \, mol^{-1}$

An electric heater of power $600 \, W$ takes $8 \, \text{minutes}$ to evaporate $80 \, mL$ of water. The enthalpy of vaporization of water is ......... $kJ \, mol^{-1}$.

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$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?

Enthalpy of hydrogenation of one mole of benzene to cyclohexane is
$[$Resonance energy of benzene $= -150.4 \ kJ / mol$.
Enthalpy of hydrogenation of cyclohexene $= -119.5 \ kJ / mol$ $]$