If Δ H0 and Δ S0 , in which of the following cases, can a reaction be spontaneous?

Question

If Δ H>0 and Δ S>0 , in which of the following cases, can a reaction be spontaneous? (A)  Δ H>T.Δ S  (B)  Δ H=T.Δ S  (C)  Δ H < T.Δ S  (D) The reaction will be non-spontaneous

Tardigrade Admin · Accepted Answer

From Gibbs Helmholtz equation, Δ G=Δ H-T . Δ S For the reaction to be spontaneous, Δ G must be negative, hence as Δ H and T . Δ S, both are positive, then T Δ S should be greater than Δ H. i.e., Δ H < T . Δ S

Q. If $Δ H > 0$ and $Δ S > 0$ , in which of the following cases, can a reaction be spontaneous?

$Δ H > T .Δ S$

$Δ H = T .Δ S$

$Δ H < T .Δ S$

The reaction will be non-spontaneous

From Gibbs Helmholtz equation,
$Δ G = Δ H - T .Δ S$
For the reaction to be spontaneous, $Δ G$ must be negative, hence as $Δ H$ and $T .Δ S$ , both are positive, then $T Δ S$ should be greater than $Δ H$ . i.e.,
$Δ H < T .Δ S$

Q. If ΔH>0 and ΔS>0 , in which of the following cases, can a reaction be spontaneous?

ΔH>T.ΔS

ΔH=T.ΔS

ΔH<T.ΔS