Gibb's Helmholtz equation

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Question

For a particular process when $ΔH = 60 kJ / mole and Δ S=200J {Kmole}^{- 1}$ then the process is non-spontaneous at

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Solution

At equilibrium, $ΔG = 0$
$∴ ΔH - TΔS = 0$
$ΔH = TΔS$
$T_{eq} = \frac{60 \times 10^{3}}{200}$ =300 K
$ΔG = + ve - T (+ ve)$
Process is spontaneous when ‘T’ is greater than $T_{eq}$ (300K)
Process is non-spontaneous when ‘T’ is lesser than $T_{eq}$ (300K)

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