- 1(current)
Q. No.For a given reaction, if ΔH = 35.5 kJ/mol and ΔS = 83.6 J/K·mol, at what temperature is the reaction spontaneous?
(Assume ΔH and ΔS remain constant with temperature.)
| 1. | T < 425 K | 2. | T > 425 K |
| 3. | All temperatures | 4. | T > 298 K |
Subtopic: Gibbs Energy Change |
75%
Level 2: 60%+
NEET - 2017
Hints
For a given reaction, ∆H = 35.5 kJ mol–1 and ∆S = 83.6 J K–1 mol–1. The reaction is spontaneous at:
[Note: Assume that ∆H and ∆S do not vary with temperature]
1. T > 425K
2. All temperatures
3. T > 298K
4. T < 425K
Subtopic: Gibbs Energy Change |
76%
Level 2: 60%+
NEET - 2017
Hints
Find the thermodynamic condition required for a reaction to be spontaneous at all temperatures.
1. ΔH > 0 and ΔS < 02. ΔH < 0 and ΔS > 0
3. ΔH < 0 and ΔS < 0
4. ΔH > 0 and ΔS > 0
Subtopic: Gibbs Energy Change |
80%
Level 1: 80%+
NEET - 2016
Hints
What is the correct thermodynamic conditions for a spontaneous reaction at all temperatures?
1. H > 0 and S< 0
2. H < 0 and S> 0
3. H < 0 and S< 0
4. H > 0 and S = 0
1. H > 0 and S< 0
2. H < 0 and S> 0
3. H < 0 and S< 0
4. H > 0 and S = 0
Subtopic: Gibbs Energy Change |
85%
Level 1: 80%+
NEET - 2016
Hints
- 1(current)
Q. No.
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