Two moles of an ideal gas is heated at a constant pressure of one atmosphere from 27C to 127C. If then q and for the process are respectively:
1. 6362.8 J, 4700 J
2. 3037.2 J, 4700 J
3. 7062.8 J, 5400 J
4. 3181.4 J, 2350 J
Calculate (in kJ/mol) for from the and the values provided at 27C
1. -2258.1 kJ/mol
2. -1129.05 kJ/mol
3. -964.35 kJ/mol
4. None of the above
The standard heat of combustion of propane is –2220.1 kJ mol–1. The standard heat of vaporisation of liquid water is 44.0 kJ mol–1. The enthalpy change for the reaction is–
C3H8 (g) + 5O2 (g) 3CO2 (g) + 4H2O(g)
1. | –2220.1 kJ | 2. | –2044.1 kJ |
3. | –2396.1 kJ | 4. | –2176.1 kJ |
Consider the following reaction,
S + O2 SO2, H = – 298.2 kJ mole–1
SO2 + 1/2 O2 SO3, H = – 98.7kJ mole–1
SO3 + H2O H2SO4 , H = – 130.2 kJ mole–1
H2 + 1/2 O2 H2O, H = – 287.3 kJ mole–1
the enthalpy of formation of H2SO4 at 298 K will be–
1. | – 814.4 kJ mole–1 | 2. | + 814.4 kJ mole–1 |
3. | – 650.3 kJ mole–1 | 4. | – 433.7 kJ mole–1 |
2.1 g of Fe combines with S evolving 3.77 kJ. The heat of formation of FeS in kJ/mole is–
1. | – 3.77 | 2. | – 1.79 |
3. | – 100.5 | 4. | None of the above |
The bond energy of H—H and Cl-Cl is 430 kJ mol-1 and 240 kJ mol-1 respectively
and ΔHf for HCl is -90 kJ mol-1. The bond enthalpy of HCl is:
1. 290
2. 380
3. 425
4. 245
1. 1.968 V
2. 2.0968 V
3. 1.0968 V
4. 0.0968 V
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
From the following bond energies:
H—H bond energy: 431.37 kJ mol-1
C=C bond energy: 606.10 kJ mol-1
C—C bond energy: 336.49 kJ mol-1
C—H bond energy: 410.50 kJ mol-1
Enthalpy for the reaction,
will be:
1. | 1523.6 kJ mol-1 | 2. | -243.6 kJ mol-1 |
3. | -120.0 kJ mol-1 | 4. | 553.0 kJ mol-1 |
Pairs correctly represent intensive property among the following is:
1. Entropy, Gibb’s energy
2. Enthalpy, Heat capacity
3. Electrode potential, Vapour pressure
4. Resistance, Conductance