Q. No.The heat of combustion of carbon to CO2 is –393.5 KJ/mol. The heat released 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
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
\(\mathrm{Ag_2 CO_3 (s) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)}\)
[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. \(7.9 \times 10^{-2}\)
Enthalpy of combustion: ΔHc(CH₄) = 890 kJ mol⁻¹, ΔHc(C₃H₈) = 2220 kJ mol⁻¹.
| 1. | 38 | 2. | 317 |
| 3. | 477 | 4. | 32 |
| (i) | C(graphite) + O2(g) \(\rightarrow\) CO2(g); \(\Delta_{r}\)H° = x kJ mol–1 |
| (ii) | Cgraphite + 1/2 O2(g) \(\rightarrow\) CO(g); \(\Delta_{r}\)H° = y kJ mol–1 |
| (iii) | CO(g) + 1/2 O2(g) \(\rightarrow\) CO2(g); \(\Delta_{r}\)H° = z kJ mol–1 |
| 1. | z = x + y | 2. | x = y + z |
| 3. | y = 2z – x | 4. | x = y – z |
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) |
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 standard enthalpy of vaporization for water at 100 oC is 40.66 kJ mol–1. The internal energy of vaporization of water at 100 oC (in kJ mol–1) is:
(Assume water vapour behaves like an ideal gas.)
| 1. | +37.56 | 2. | –43.76 |
| 3. | +43.76 | 4. | +40.66 |
Equal volumes of two monoatomic gases, A and B, at same temperature and pressure are mixed. The ratio of specific heats (Cp/Cv) of the mixture will be:
| 1. | 1.50 | 2. | 3.3 |
| 3. | 1.67 | 4. | 0.83 |
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