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For the process $A (g) + B (g) \to_{}^{} C (g)$ , $Δ^{o} H = - 30.3 KJ / mole$ . If $S_{A}^{o} {, S}_{B}^{o}$ and $S_{C}^{o}$ are ${144 JK}^{- 1} {mole}^{- 1}, 81 {JK}^{- 1} {mole}^{- 1}$ and $125 {JK}^{- 1} {mole}^{- 1}$ respectively. Is the process spontaneous?

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No, $Δ^{o} G = + 0.5 KJ / mole$

Yes, $Δ^{o} G = - 60.1 KJ / mole$

No, $Δ^{o} G = + 60.1 KJ / mole$

Yes, $Δ^{o} G = - 0.5 KJ / mole$

answer is C.

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Detailed Solution

$Δ^{o} S = 125 - (144 + 81) - 100 {JK}^{- 1} {mole}^{- 1}$

$= - 0.1 {KJ K}^{- 1} {mole}^{- 1}$

$Δ^{o} G = [- 30.3 - 298 (- 0.1)] KJ / mole$

$= - 0.5 KJ / mole$

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