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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A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5 atm from an initial volume of 2.50 L to a final volume of 4.50 L. The change in internal energy U of the gas in joules will be

(1) 1136.25 J

(2) - 500 J

(3) - 505 J

(4) + 515 J

Subtopic:  First Law of Thermodynamics |
 66%
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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A gas is allowed to expand in a well-insulated container against a constant external pressure of 2.5atm from an initial volume of 2.50 L to a final volume of 4.50L. The change in internal energy U of the gas in joules will be:

1. –500J 2. –505J
3. –506J 4. –508J
Subtopic:  First Law of Thermodynamics |
From NCERT
NEET - 2017
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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
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The heat of combustion of carbon to CO2 is –393.5 KJ/mol. The heat released upon the formation of 35.2 g of CO2 from carbon and oxygen gas is:
1. –315 KJ
2. +315 KJ
3. –630 KJ
4. +630 KJ

Subtopic:  Thermochemistry |
 74%
From NCERT
NEET - 2015
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The correct statement for a reversible process in a state of equilibrium is:
1. G = – 2.30RT log K
2. G = 2.30RT log K
3. Go = – 2.30RT log K
4. Go = 2.30RT log K

Subtopic:  Gibbs Energy Change |
 80%
From NCERT
NEET - 2015
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Given the Gibbs free energy change, ΔG=+63.3 kJ, for the following reaction, 
Ag2CO3(s)2Ag+(aq)+CO32(aq)
Ksp of Ag2CO3(s) in water at 25º C is:
(R = 8.314 JK–1 mol–1)
1. 3.2×1026
2. 8.0×1012
3. 2.9×103
4. 7.9×102
Subtopic:  Gibbs Energy Change |
 61%
From NCERT
AIPMT - 2014
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For the reaction:
X2O4(l)2XO2(g)
with the given values ΔU=2.1kcal and ΔS=20cal K1 at 300K, what is the value of ΔG?

1. 2.7 kcal
2. –2.7 kcal
3. 9.3 kcal
4. –9.3 kcal

Subtopic:  Gibbs Energy Change |
 78%
From NCERT
AIPMT - 2014
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In which of the following reactions, the standard reaction entropy change
(S0) is positive, and standard Gibb's energy change
(G0) decreases sharply with increasing temperature?

1. C(graphite) + 12O2(g) → CO(g)
2. CO(g) + 12O2(g) → CO2(g)
3. Mg(s) + 12O2(g) → MgO(s)
4. 12C(graphite) + 12O2(g) → 12CO2(g)

Subtopic:  Gibbs Energy Change |
 71%
From NCERT
AIPMT - 2012
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