[letr]

7. The reaction to produce a drug has a ΔH value of –10.07 kJmol-1 and a ΔS value of 42.12 Jmol-1 K-1
at 20°C. State whether this reaction will proceed spontaneously at 25°C and explain why. (5 marks)

ΔG = ΔH – TΔS (where ΔH = -10.07 kJ mol-1, ΔS = 42.12 J mol-1 K-1 and T = 293K)
ΔG = 10.96- 2.95 = +8.01 kJ mol-1 (2 s.f.).
Reaction does not proceed as ΔG is positive

[charco]

(Original post by letr)
7. The reaction to produce a drug has a ΔH value of –10.07 kJmol-1 and a ΔS value of 42.12 Jmol-1 K-1
at 20°C. State whether this reaction will proceed spontaneously at 25°C and explain why. (5 marks)

ΔG = ΔH – TΔS (where ΔH = -10.07 kJ mol-1, ΔS = 42.12 J mol-1 K-1 and T = 293K)
ΔG = 10.96- 2.95 = +8.01 kJ mol-1 (2 s.f.).
Reaction does not proceed as ΔG is positive

The entropy change is positive and the enthalpy change is negative. This means that it is IMPOSSIBLE to get a positive value for ΔG

The reaction is spontaneous at all temperatures...