The ΔG vs T plot shown is for a reaction with ΔH<0 and ΔS<0.
For a reaction with ΔH < 0 and ΔS < 0, the ΔG vs T line slopes upward. What does this imply?
- A
Always spontaneous
- B
Spontaneous at high T only
- Ccheck_circle
Spontaneous at low T; non-spontaneous at high T
- D
Always non-spontaneous
Explanation
ΔG = ΔH - TΔS. With ΔH<0 and ΔS<0, the -TΔS term grows positive with T, so ΔG eventually exceeds 0.