(B) The standard free energy change is calculated using the formula: $\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$. Given: $\Delta H^\circ = 58.

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(B) The standard free energy change is calculated using the formula: $\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$. Given: $\Delta H^\circ = 58.04 \ kJ$,$\Delta S^\circ = 176.7 \ J/K = 0.1767 \ kJ/K$,and $T = 25 + 273 = 298 \ K$. Substituting the values: $\Delta G^\circ = 58.04 \ kJ - (298 \ K \times 0.1767 \ kJ/K)$. $\Delta G^\circ = 58.04 \ kJ - 52.66 \ kJ = 5.38 \ kJ$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

The standard enthalpy for the decomposition of $N_2O_5$ to $NO_2$ is $58.04 \ kJ$ and standard entropy of this reaction is $176.7 \ J/K$. The standard free energy change for this reaction at $25 \ ^oC$ is .................. $kJ$.

A
$-5.38$
B
$5.38$
C
$53.8$
D
$-53.8$

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Class 11 Questions

Class 11

Chemistry Questions

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Thermodynamics

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Free energy and Work

Which of the following conditions will oppose or prevent a reaction from occurring?

Easy

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For the reaction $Ag_2O_{(s)} \rightarrow 2Ag_{(s)} + 1/2 O_{2_{(g)}}$,the value of $\Delta H = 30.56 \, kJ \, mol^{-1}$ and $\Delta S = 66 \, J \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the change in free energy for the reaction be zero?

Medium

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For water,the value of $\Delta H_{vap}$ is $40.73 \, kJ \, mol^{-1}$ and the value of $\Delta S_{vap}$ is $109 \, J \, K^{-1} \, mol^{-1}$. At what temperature will water be in equilibrium with its vapor?

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For a reaction at $25 \, ^oC$,the enthalpy change and entropy change are $-11.7 \times 10^3 \, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} \, K^{-1}$ respectively. What is the Gibbs free energy in $kJ$?

Medium

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For a spontaneous change,free energy change $\Delta G$ is

Easy

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The standard enthalpy for the decomposition of $N_2O_5$ to $NO_2$ is $58.04 \ kJ$ and standard entropy of this reaction is $176.7 \ J/K$. The standard free energy change for this reaction at $25 \ ^oC$ is .................. $kJ$.

Similar Questions

Which of the following conditions will oppose or prevent a reaction from occurring?

For the reaction $Ag_2O_{(s)} \rightarrow 2Ag_{(s)} + 1/2 O_{2_{(g)}}$,the value of $\Delta H = 30.56 \, kJ \, mol^{-1}$ and $\Delta S = 66 \, J \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the change in free energy for the reaction be zero?

For water,the value of $\Delta H_{vap}$ is $40.73 \, kJ \, mol^{-1}$ and the value of $\Delta S_{vap}$ is $109 \, J \, K^{-1} \, mol^{-1}$. At what temperature will water be in equilibrium with its vapor?

For a reaction at $25 \, ^oC$,the enthalpy change and entropy change are $-11.7 \times 10^3 \, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} \, K^{-1}$ respectively. What is the Gibbs free energy in $kJ$?

For a spontaneous change,free energy change $\Delta G$ is

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