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 |
 78%
From NCERT
NEET - 2015
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Given the Gibbs free energy change, \(\Delta G^\circ=+63.3~kJ,\) for the following reaction, 
\(Ag_2 CO_3 (g) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)\)
\(K_{sp}\) of \(Ag_2CO_3 (s) \) in water at 25º C is (R = 8.314 JK-1 mol-1)

1. \(3.2 \times 10^{26}\)
2. \(8.0 \times 10^{-12}\)
3. \(2.9 \times 10^{-3}\)
4. \(7.9 \times 10^{-2}\)
Subtopic:  Gibbs Energy Change |
 60%
From NCERT
AIPMT - 2014
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Given the reaction: 
X2O4(l) → 2XO2(g) 
ΔU = 2.1 kcal, ΔS = 20 cal K–1 at 300 K 
The value of ΔG is:
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) + \(\frac{1}{2}\)O2(g) → CO(g)
2. CO(g) + \(\frac{1}{2}\)O2(g) → CO2(g)
3. Mg(s) + \(\frac{1}{2}\)O2(g) → MgO(s)
4. \(\frac{1}{2}\)C(graphite) + \(\frac{1}{2}\)O2(g) → \(\frac{1}{2}\)CO2(g)

Subtopic:  Gibbs Energy Change |
 69%
From NCERT
AIPMT - 2012
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Standard entropies of X2, Y2 and XY3 are 60, 40 and 50JK-1mol-1 respectively. For the reaction 
12X2 + 32Y2   XY3 ; H = -30 kJ to be at equilibrium, the temperature should be:

1. 750 K

2. 1000 K

3. 1250 K

4. 500 K

Subtopic:  Gibbs Energy Change |
 78%
From NCERT
AIPMT - 2010
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For vaporization of water at 1 atmospheric pressure, the values of ∆H and ∆S are 40.63 kJ mol–1 and 108.8 JK–1 mol–1, respectively. The temperature when Gibbs energy change (∆G) for this transformation will be zero, is:

1. 393.4 K

2. 373.4 K

3. 293.4 K

4. 273.4 K

Subtopic:  Gibbs Energy Change |
 78%
From NCERT
AIPMT - 2010
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Match List – I (Equations) with List – II (Type of processes) and select the correct option.

List – I List – II
Equation  Type of processes
(a) Kp > Q  (i) Non-spontaneous
(b) ∆Gº < RT ln Q  (ii) Equilibrium
(c) Kp = Q  (iii) Spontaneous and endothermic
(d) T > \(\frac{\Delta H}{\Delta S}\) (iv) Spontaneous
 
Options: (a) (b) (c) (d)
1. (iii) (iv) (ii) (i)
2. (iv) (i) (ii) (iii)
3. (ii) (i) (iv) (iii)
4. (i) (ii) (iii) (iv)
Subtopic:  Spontaneity & Entropy | Gibbs Energy Change |
 63%
From NCERT
AIPMT - 2010
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The values of ΔH and ΔS for the given reaction are 170 kJ and 170 JK-1, respectively.
C(graphite) + CO2(g)→2CO(g) 
This reaction will be spontaneous at:

1. 710 K
2. 910 K
3. 1110 K
4. 510 K

Subtopic:  Gibbs Energy Change |
 88%
From NCERT
AIPMT - 2009
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Which of the following are not state functions? 
(I) q + W 
(II) q 
(III) W 
(IV) H - TS

1. (I) and (IV)
2. (II), (III) and (IV)
3. (I), (II) and (III)
4. (II) and (III)
Subtopic:  Gibbs Energy Change |
 75%
From NCERT
AIPMT - 2008
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For the gas phase reaction, 
 PCl5(g)PCl3(g)+Cl2(g)
which of the following conditions is correct?

1. ΔH = 0 and ΔS < 0

2. ΔH > 0 and ΔS > 0

3. ΔH < 0 and ΔS < 0

4. ΔH > 0 and ΔS < 0

Subtopic:  Gibbs Energy Change |
 80%
From NCERT
AIPMT - 2008
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