For a particular reversible reaction at temperature T,ΔH and ΔS were found to be both positive. If Te is the temperature at equilibrium, the reaction would be spontaneous when

For a particular reversible reaction at temperature $T, Δ H$ and $Δ S$ were found to be both positive. If $T_{e}$ is the temperature at equilibrium, the reaction would be spontaneous when

A
$T = T_{e}$
B
$T_{e} > T$
C
$T > T_{e}$
D
$T_{e}$ is 5 times $T$

Solution:

Since $Δ G = Δ H - T Δ G$ , we have

Reactions at equilibrium: $Δ G = Δ H - T_{e} Δ S = 0$

For a reaction to be spontaneous: $Δ G = Δ H - T Δ S < 0$

$Δ G$ will be negative provided $T > T_{e}$ as both $Δ H$ and $Δ S$ are positive.

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