For a reaction at 25,^oC,the enthalpy change | vedclass

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

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Non-spontaneous

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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: $\Delta H = -11.7 	imes 10^3 \, J \, mol^{-1}$,$\Delta S = -105 \, J \, mol^{-1} K^{-1}$,and $T = 25 + 273 = 298 \, K$. Substituting the values: $\Delta G = (-11.7 	imes 10^3) - (298 	imes -105)$. $\Delta G = -11700 + 31290 = +19590 \, J \, mol^{-1}$. Since $\Delta G > 0$,the reaction is non-spontaneous.

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:

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