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 |
 74%
From NCERT
NEET - 2017
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For a given reaction, ∆H = 35.5 kJ mol–1 and ∆S = 83.6 J K–1 mol–1. The reaction is spontaneous at:
(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%
From NCERT
NEET - 2017
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NEET 2026 - Target Batch - Vital
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The correct thermodynamic conditions for the spontaneous reaction at all temperatures is

(a)H>0andS<0
(b)H<0andS>0
(c)H<0andS<0
(d)H<0andS=0

Subtopic:  Gibbs Energy Change |
 80%
From NCERT
NEET - 2016
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The correct thermodynamic conditions for a spontaneous reaction at all temperatures is:
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%
From NCERT
NEET - 2016
To view explanation, please take trial in the course.
NEET 2026 - Target Batch - Vital
Hints
To view explanation, please take trial in the course.
NEET 2026 - Target Batch - Vital