Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be:
1. 3 Joules
2. 9 Joules
3. Zero
4. Infinite
The following two reactions are known
The value of H for the following reaction
is:
1. -43.3 kJ
2. -10.3 kJ
3. +6.2 kJ
4. +10.3 kJ
Match List – I (Equations) with List – II (Type of processes) and select the correct option.
List – I | List – II | ||
Equation | Type of processes | ||
(a) | Kp > Q | (i) | Non-spontaneous |
(b) | ∆Gº < RT ln Q | (ii) | Equilibrium |
(c) | Kp = Q | (iii) | Spontaneous and endothermic |
(d) | T > \(\frac{\Delta H}{\Delta S}\) | (iv) | Spontaneous |
Options: | (a) | (b) | (c) | (d) |
1. | (iii) | (iv) | (ii) | (i) |
2. | (iv) | (i) | (ii) | (iii) |
3. | (ii) | (i) | (iv) | (iii) |
4. | (i) | (ii) | (iii) | (iv) |
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
For vaporization of water at 1 atmospheric pressure, the values of ∆H and ∆S are 40.63 kJ mol–1 and 108.8 JK–1 mol–1, respectively. The temperature when Gibbs energy change (∆G) for this transformation will be zero, is:
1. 393.4 K
2. 373.4 K
3. 293.4 K
4. 273.4 K
Consider the following processes:
∆H (kJ/mol)
½ A → B + 150
3B → 2C + D –125
E + A → 2D +350
For B + D → E + 2C, ∆H will be-
1. 325 kJ/mol
2. 525 kJ/mol
3. –175 kJ.mol
4. –325 kJ/mol
(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 combustion of H2, cyclohexene (C6H10) and cyclohexane (C6H12) are -241, -3800 and -3920 kJ per mol respectively. Heat of hydrogenation of cyclohexene is:
1. -121 kJ per mol
2. +121 kJ per mol
3. +242 kJ per mol
4. -242 kJ per mol
The enthalpy and entropy change for the reaction: Br2 (l) + Cl2 (g) →2BrCl(g), are 30kJ mol-1 and 105 JK-1 mol-1 respectively. The temperature at which the reaction will be in equilibrium is:
1. 285.7 K
2. 273 K
3. 450 K
4. 300 K