Which of the following statements is correct for a reversible process in a state of equilibrium?
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 |
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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 |
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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 |
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In which of the following reactions, standard reaction entropy change $\left(∆{S}^{0}\right)$ is positive and standard Gibb's energy change $\left(∆{G}^{0}\right)$ decreases sharply with increasing temperature?

1. $C\left(graphite\right)+\frac{1}{2}{O}_{2}\left(g\right)\to CO\left(g\right)$

2. $CO\left(g\right)+\frac{1}{2}{O}_{2}\left(g\right)\to C{O}_{2}\left(g\right)$

3. $Mg\left(s\right)+\frac{1}{2}{O}_{2}\left(g\right)\to MgO\left(s\right)$

4. $\frac{1}{2}C\left(graphite\right)+\frac{1}{2}{O}_{2}\left(g\right)\to \frac{1}{2}C{O}_{2}\left(g\right)$

Subtopic:  Gibbs Energy Change |
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Standard entropies of X2, Y2 and XY3 are 60, 40 and 50JK-1mol-1 respectively. For the reaction
to  be at equilibrium, the temperature should be

1. 750 K

2. 1000 K

3. 1250 K

4. 500 K

Subtopic:  Gibbs Energy Change |
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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 |
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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 > $\frac{∆H}{∆S}$                       (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 |
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The values of ΔH and ΔS for the reaction, C(graphite) + CO2(g)→2CO(g) are 170 kJ and 170 JK-1, respectively. This reaction will be spontaneous at
1. 710 K
2. 910 K
3. 1110 K
4. 510 K

Subtopic:  Gibbs Energy Change |
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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 |
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For the gas phase reaction,
${\mathrm{PCl}}_{5}\left(\mathrm{g}\right)⇌{\mathrm{PCl}}_{3}\left(\mathrm{g}\right)+{\mathrm{Cl}}_{2}\left(\mathrm{g}\right)$
which of the following conditions are 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 |
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