A. | A liquid evaporates to vapour. |
B. | Temperature of a crystalline solid lowered from \(130~\text{K}\) to \(0~\text{K}.\) |
C. | \(2 \mathrm{NaHCO}_{3(\mathrm{~s})} \rightarrow \mathrm{Na}_2 \mathrm{CO}_{3(\mathrm{~s})}+\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}\) |
D. | \(\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{Cl}_{(\mathrm{g})}\) |
1. | \(\text { A, B and D }\) | 2. | \(\text { A, C and D }\) |
3. | \(\text { C and D }\) | 4. | \(\text { A and C }\) |
For irreversible expansion of an ideal gas under isothermal condition, the correct option is :
1.
2.
3.
4.
For the reaction, 2Cl(g) Cl2(g), the correct option is:
1.
2.
3.
4.
If for a certain reaction is 30 kJ mol–1 at 450 K, the value of (in JK–1 mol–1) for which the same reaction will be spontaneous at the same temperature is:
1. 70
2. –33
3. 33
4. –70
For a sample of a perfect gas when its pressure is changed isothermally from Pi to Pf, the entropy change is given by:
1.
2.
3.
4.
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) |
A reaction occurs spontaneously if:
1. T∆S > ∆H and ∆H is +ve and ∆S are –ve
2. T∆S = ∆H and both ∆H and ∆S are +ve
3. T∆S < ∆H and both ∆H and ∆S are +ve
4. T∆S > ∆H and both ∆H and ∆S are +ve
Which of the following pairs of chemical reactions is certain to result in a spontaneous reaction:
1. Endothermic and decreasing disorder
2. Exothermic and increasing disorder
3. Endothermic and increasing disorder
4. Exothermic and decreasing disorder
Considering entropy (S) as a thermodynamic parameter, the criterion for the spontaneity of any process is:
1.
2.
3.
4.
What is the entropy change (in JK–1 mol–1) when one mole of ice is converted into water at 0 ºC? (The enthalpy change for the conversion of ice to liquid water is 6.0 KJ mol–1 at 0 ºC)
1. | 20.13 | 2. | 2.013 |
3. | 2.198 | 4. | 21.98 |