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
An ideal gas is expanded irreversibly against 10 bar pressure from 20 litres to 30 litres. Calculate 'w' if the process is isoenthalpic.
1. | 0 | 2. | +100J |
3. | -100 J | 4. | -10 kJ |
The standard enthalpy of combustion at of hydrogen, cyclohexene (C6H10), and cyclohexane (C6H12) are -241, -3800 and -3920 kJ mol-1, respectively. Calculate the standard enthalpy of hydrogenation of cyclohexene.
1. | -131 kJ mol-1 | 2. | -155 kJ mol-1 |
3. | -167 kJ mol-1 | 4. | -121 kJ mol-1 |
4.8 g of C(diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of the formation of gaseous carbon is 725 kJ/mol. The energy required for the given process will be:
(i)
(ii)
1. | 725, 727 | 2. | 727, 725 |
3. | 725, 723 | 4. | None of the above |
As an isolated box, equally partitioned, contains two ideal gasses A and B as shown:
When the partition is removed, the gases mix. The changes in enthalpy and entropy in the process, respectively, are
1. Zero, positive
2. Zero, negative
3. Positive, zero
4. Negative, zero
The for vaporization of a liquid is \(20 \mathrm{~kJ} / \mathrm{mol}.\) Assuming ideal behaviour, the change in internal energy for the vaporization of \(1 \mathrm{~mol}\) of the liquid at \(60^{\circ} \mathrm{C}\) and 1 bar is close to:
1. | \(13.2 \mathrm{~kJ} / \mathrm{mol} \) | 2. | \(17.2 \mathrm{~kJ} / \mathrm{mol} \) |
3. | \(19.5 \mathrm{~kJ} / \mathrm{mol} \) | 4. | \(20.0 \mathrm{~kJ} / \mathrm{mol}\) |
The entropy change in the isothermal reversible expansion of 2 moles of an ideal gas from 10 to 100 L at 300 K is
1.
2.
3.
4.
An ideal gas expands isothermally from at 300 K against a constant pressure of . The work done by the gas is:
1. | +270 kJ | 2. | –900 J |
3. | +900 kJ | 4. | –900 kJ |
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 |
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 |