- 1(current)
Q. No.\(\mathrm{2H_2(g) + O_2(g) \rightarrow 2H_2O(g); ~\Delta_rH^\circ = -483.64~ kJ }\)
What is the enthalpy change (in KJ) for the decomposition of one mole of water?
| 1. | 120.9 | 2. | 241.82 |
| 3. | 18 | 4. | 100 |
At standard conditions, if the change in the enthalpy for the following reaction is –109 kJ mol–1
H2(g)+Br2(g)2HBr(g) and the bond energy of H2 and Br2 is 435 kJ mol–1 and 192 kJ mol–1 respectively, what is the bond energy (in kJ mol–1) of HBr?
| 1. | 368 | 2. | 736 |
| 3. | 518 | 4. | 259 |
The bond dissociation energies of X2 , Y2 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
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 |
Enthalpy of combustion: ΔHc(CH₄) = 890 kJ mol⁻¹, ΔHc(C₃H₈) = 2220 kJ mol⁻¹.
| 1. | 38 | 2. | 317 |
| 3. | 477 | 4. | 32 |
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) |
- 1(current)
Q. No.
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