# 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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Which of the following statements is correct for the spontaneous adsorption of a gas ?

1. $∆$S is negative and therefore, $∆$H should be highly positive
2. $∆$S is negative and therefore, $∆$H should be highly negative
3. $∆$S is positive and therefore, $∆$H should be negative
4. $∆$S is positive and therefore, $∆$H should also be highly positive

Subtopic:  Spontaneity & Entropy |
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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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The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0 oC is:

1. 10.52 cal/(mol K)

2. 21.04 cal/(mol K)

3. 5.260 cal/(mol K)

4. 0.526 cal/(mol K)

Subtopic:  Thermochemistry |
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Standard enthalpy of vaporization ${∆}_{\mathrm{vap}}{\mathrm{H}}^{0}$for water at 1000C is 40.66 Kj mol-1. The internal energy of vaporization of water at 1000C (in kJ mol-1) is
(Assume water vapour to behave like an ideal gas).

1. +37.56

1. -43.76

3. +43.76

4. +40.66

Subtopic:  Enthalpy & Internal energy |
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Which of the following is the correct option for free expansion of an ideal gas under adiabatic condition?
1.
2.
3.
4.

Subtopic:  2nd & 3rd Law of Thermodynamics |
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Given the following reaction:
4H(g) 2H2 (g)
The enthalpy change for the reaction is -869.6 kJ. The dissociation energy of the H-H bond is -
1. -869.6 kJ
2. +434.8kJ
3. +217.4kJ
4. -434.8 kJ

Subtopic:  Enthalpy & Internal energy |
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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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