Q. No.Which of the following are not state functions?
(I) q + W (II) q
(III) W (IV) H-TS
1. (I) and (IV)
2. (II), (III) and (IV)
3. (I) , (II) and (III)
4. (II) and (III)
| \(\small\text{(i)}~ \text{H}^+(aq) + \text{OH}^-(aq) \rightarrow \text{H}_2\text{O}(l); \quad \Delta H = -x_1 \text{ kJ mol}^{-1}\) |
| \(\small\text{(ii)}~ \text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l); \quad \Delta H = -x_2 \text{ kJ mol}^{-1}\) |
| \(\small\text{(iii)}~ \text{CO}_2(g) + \text{H}_2(g) \rightarrow \text{CO}(g) + \text{H}_2\text{O}(l); \quad \Delta H = -x_3 \text{ kJ mol}^{-1}\) |
| \(\small(iv)~ \text C_ 2\text H_ 5 ( g ) + \frac{5} {2} \text O_ 2 ( g ) = 2 \text C\text O_ 2 ( g ) + \text H_ 2 \text O ( l )~; ∆ H = - x_ 4~ kJ mol^ {- 1} \) |
Choose the correct option:
1. -x2 kJ mol-1
2. +x3 kJ mol-1
3. -x4 kJ mol-1
4. -x1 kJ mol-1
Identify the correct statement for the change of Gibbs free energy for a system (Gsystem) at constant temperature and pressure:
| 1. | If Gsystem > 0, the process is spontaneous |
| 2. | If Gsystem = 0, the system has attained equilibrium |
| 3. | If Gsystem = 0, the system is still moving in a particular direction |
| 4. | If Gsystem < 0, the process is not spontaneous |
The enthalpy and entropy change for the reaction :
Br2 (l) + Cl2 (g) 2BrCl (g)
are 30 kJ mol-1 and 105 J K-1 mol-1 respectively.
The temperature at which the reaction will be in equilibrium is :
| 1. | 285.7 K | 2. | 273.4 K |
| 3. | 450.9 K | 4. | 300.1 K |
The enthalpy of combustion of H2, cyclohexene (C6H10) and cyclohexane (C6H12) are -241, -3800 and -3920 kJ per mol respectively. Heat of hydrogenation of cyclohexene is:
(a) -121 kJ per mol
(b) +121 kJ per mol
(c) +242 kJ per mol
(d) -242 kJ per mol
Consider the reactionat 300K
H2(9) + Cl2(9) →2HCI(g), ΔH° = — 185 KJ
If 3 mole of H2 completely react with 3 mol of Cl2 to form Cl, U° of the reaction will be
(1) Zero
(2) –185 KJ
(3) -555 KJ
(4) None
For a perfectly crystalline solid Cpm = aT3, where a is constant. If Cpm is 0.42 J/K–mol at 10 K, molar entropy at 10 K is
1. 0.42 J/K–mol
2. 0.14 J/K–mol
3. 4.2 J/K–mol
4. zero
One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300 K then total entropy change of system in the above process is :
[R = 0.082 L atm mol–1 K–1 = 8.3 J mo1–1K–1].
(1) 0
(2) Rln (24.6)
(3) Rln (2490)
(4) Rln(24.6)
At 1000 K water vapour at 1 atm. has been found to be dissociated into H2 and O2 to the extent of 3 x 10–6 %.Calculate the free energy decrease of the system, assuming ideal behaviour.
(1) –ΔG = 90,060 cal
(2) –ΔG = 20 cal
(3) –ΔG = 480 cal
(4) –ΔG = –45760 cal
An ideal gas is taken from the same initial pressure P1 to the same final pressure P2 by three different processes. If it is known that point 1 corresponds to a reversible adiabatic and point 2 corresponds to a single stage adiabatic then
(1) Point 3 may be a two stage adiabatic.
(2) the average K.E. of the gas is maximum at point 1
(3) Work done by surrounding in reaching point number '3' will be maximum
(4) If point4 and point 5 lie along a reversible isotherm then T5 < T1.
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