Q. No.2A (g) + B (g) → 2D (g)
\(ΔU^⊖\)=−10 \(kJ mol^{−1}\) and \(ΔS^⊖\)=−44 \(J K^{−1}\) at 298 K.
Identify the correct option with \(ΔG^⊖\) for the reaction and spontaneity of the reaction at 298 K.
(Given : R=\(8.31 ~J mol^{−1} K^{−1}\))
| 1. | −1.635 kJ mol−1, spontaneous |
| 2. | +0.63568 kJ mol−1, non-spontaneous |
| 3. | −0.63568 kJ mol−1, spontaneous |
| 4. | +1.635 kJ mol−1, non-spontaneous |
Hydrolysis of sucrose is given by the following reaction
Sucrose + H2O Glucose + Fructose
If the equilibrium constant (Kc) is 21013 at 300 K, the value of at the same temperature will be:
1. 8.314 J mol–1 K–1300 Kln (21013)
2. 8.314 J mol–1 K–1300 Kln (31013)
3. –8.314 J mol–1 K–1300 Kln (41013)
4. –8.314 J mol–1 K–1300 Kln (21013)
Which of the following processes shows a decrease in entropy?
1. \(2 \text H \left(g\right)\rightarrow\text H_{2} \left(g\right)\)
2. Evaporation of water
3. Expansion of a gas at a constant temperature
4. Sublimation of a solid to a gas
For a given reaction, ∆H = 35.5 kJ mol–1 and ∆S = 83.6 J K–1 mol–1. The reaction is spontaneous at:
[Note: Assume that ∆H and ∆S do not vary with temperature]
1. T > 425K
2. All temperatures
3. T > 298K
4. T < 425K
1. H > 0 and S< 0
2. H < 0 and S> 0
3. H < 0 and S< 0
4. H > 0 and S = 0
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
\(\mathrm{Ag_2 CO_3 (s) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)}\)
[Given: \(\text R = 8.314 \text J\text K^{–1} \text {mol}^{–1}\) ; \(\Delta \text G^\circ=+63.3~\text{kJ}\) ]
1. \(3.2 \times 10^{26}\)
2. \(8.0 \times 10^{-12}\)
3. \(2.9 \times 10^{-3}\)
4. \(7.9 \times 10^{-2}\)
For the reaction:
\(\mathrm{X}_2 \mathrm{O}_4(l) \rightarrow 2 \mathrm{XO}_2(g)\)
with the given values \(\Delta U = 2.1 \, \text{kcal}\) and \(\Delta S = 20 \, \text{cal K}^{-1}\) at \(300 \, \text{K}\), what is the value of \(\Delta G\)?
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
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