For a spontaneous reaction, which of the following condition is correct, at all temperatures?

Question

For a spontaneous reaction, which of the following condition is correct, at all temperatures? (A) Δ H<0, Δ S<0 (B) Δ H>0, Δ S<0 (C) Δ H<0, Δ S>0 (D) Δ H>0, Δ S>0

Tardigrade Admin · Accepted Answer

For a reaction, to be spontaneous, Δ G (free energy change) must be negative. Δ G is given by Gibbs-Helmoltz equation, which is Δ G=Δ H-T⋅ Δ S Hence, from this equation it follows that Δ H will be negative at all temperature if, Δ H=- ve and Δ S=+ve i.e., Δ H<0 and Δ S>0

Q. For a spontaneous reaction, which of the following condition is correct, at all temperatures?

$Δ H < 0, Δ S < 0$

$Δ H > 0, Δ S < 0$

$Δ H < 0, Δ S > 0$

$Δ H > 0, Δ S > 0$

Q. For a spontaneous reaction, which of the following condition is correct, at all temperatures?

ΔH<0,ΔS<0

ΔH>0,ΔS<0

ΔH<0,ΔS>0

ΔH>0,ΔS>0

For a reaction, to be spontaneous, ΔG (free energy change) must be negative. ΔG is given by Gibbs-Helmoltz equation, which is ΔG=ΔH−T⋅ΔS Hence, from this equation it follows that ΔH will be negative at all temperature if, ΔH=−ve and ΔS=+ve i.e., ΔH<0 and ΔS>0

$Δ H < 0, Δ S < 0$

$Δ H > 0, Δ S < 0$

$Δ H < 0, Δ S > 0$

$Δ H > 0, Δ S > 0$