Q. No.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
\(Ag_2 CO_3 (g) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)\)
\(K_{sp}\) 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. \(7.9 \times 10^{-2}\)
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
In which of the following reactions, the standard reaction entropy change
is positive, and standard Gibb's energy change
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) |
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
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
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) |
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
(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)
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
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