Q. No.A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5atm from an initial volume of 2.50 L to a final volume of 4.50L. The change in internal energy U of the gas in joules will be:
1. -500J
2. -505J
3. -506J
4. -508J
1. -500J
2. -505J
3. -506J
4. -508J
The bond dissociation energies of and XY are in the ratio of 1 : 0.5 : 1. ∆H for the formation of XY is –200 kJ mol–1. The bond dissociation energy of X2 will be
1. 200 kJ mol–1
2. 100 kJ mol–1
3. 800 kJ mol–1
4. 400 kJ mol–1
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 heat of combustion of carbon to CO2 is -393.5 KJ/mol. The heat changed upon the formation of 35.2 g of CO2 from carbon and oxygen gas is:
1. -315 KJ
2. +315 KJ
3. -630 KJ
4. +630 KJ
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. \(7.9 \times 10^{-2}\)
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 |
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) |
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)
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