Values of Δ H and Δ S for five different reactions are given below: Reaction Δ H ( kJ mol -1) Δ S( J K -1 mol-1) I +98.0 +14.8 II -55.5 -84.8 III +28.3 -17.0 IV -40.5 +24.6 On the basis of these values predict which one of these will be spontaneous at all temperatures?

Question

Values of Δ H and Δ S for five different reactions are given below: Reaction Δ H ( kJ mol -1) Δ S( J K -1 mol-1) I +98.0 +14.8 II -55.5 -84.8 III +28.3 -17.0 IV -40.5 +24.6 On the basis of these values predict which one of these will be spontaneous at all temperatures? (A) Reaction I (B) Reaction II (C) Reaction III (D) Reaction IV

Tardigrade Admin · Accepted Answer

For reaction IV, Δ H=- ve and Δ S=+ ve, hence Δ G=- ve at all temperatures.

Reaction	$Δ H (k J m o l^{- 1})$	$Δ S (J K^{- 1} m o l^{- 1})$
I	+98.0	+14.8
II	-55.5	-84.8
III	+28.3	-17.0
IV	-40.5	+24.6

Q. Values of ΔH and ΔS for five different reactions are given below: Reaction ΔH(kJmol−1) ΔS(JK−1mol−1) I +98.0 +14.8 II -55.5 -84.8 III +28.3 -17.0 IV -40.5 +24.6 On the basis of these values predict which one of these will be spontaneous at all temperatures?

Reaction I

Reaction II

Reaction III

Reaction IV

For reaction IV, ΔH=−ve and ΔS=+ve, hence ΔG=−ve at all temperatures.

For reaction IV, $Δ H = - v e$ and $Δ S = + v e$ , hence $Δ G = - v e$ at all temperatures.