At a particular temperature and atmospheric pressure, the solid and liquid
phases of a pure substance can exist in equilibrium. Choose the terms
which define this temperature.
(a) Normal melting point
(b) Equilibrium temperature
(c) Boiling point
(d) Freezing point
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)
For the reaction N2O4(g) ⇌ 2NO2(g), the value of K(equilibrium constant) is 50 at 400 K and 1700 at 500 K. Which of the following option(s) is/are correct?
(a). | The reaction is endothermic. |
(b). | The reaction is exothermic. |
(c). | If NO2(g) and N2O4(g) are mixed at 400 K at partial pressures 20 bar and 2 bar respectively, more N2O4(g) will be formed. |
(d) | The entropy of the system increases. |
1. (a, b, d)
2. (b, c, d)
3. (b, d, a)
4. (a, c, d)
The addition of a small amount of argon at a constant volume will not affect the equilibrium of the following reaction:
1. | H2(g)+I2(g)⇌2HI(g) |
2. | PCl5(g)⇌ PCl3(g)+Cl2(g) |
3. | N2(g)+3H2(g)⇌2NH3(g) |
4. | The equilibrium will remain unaffected in all the three cases. |
At 500 K, equilibrium constant, Kc, for the following reaction is 5.
What would be the equilibrium constant Kc for the reaction?
1. 0.04
2. 0.4
3. 25
4. 2.5
On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier's principle. Consider the reaction,
Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?
1. | K will remain the same. |
2. | K will decrease. |
3. | K will increase. |
4. | K will increase initially and then decrease, when pressure is very high. |
Which of the following alternatives best describes the reaction A ⇌ B at its halfway point?
1. | \(\Delta G^{\ominus}=0\) | 2. | \(\Delta G^{\ominus}>0\) |
3. | \(\Delta G^{\ominus}<0\) | 4. | \(\Delta G^{\ominus}=-RTlnK\) |
for is and Kb for is . The pH of ammonium acetate will be:
1. 7.005
2. 4.75
3. 7.0
4. Between 6 and 7
The value of the pH of \(0.01 \) \(\text{mol dm}^{-3} \)\(\text{CH}_3\text{COOH}\) \(\left(K_a=1.74 \times 10^{-5}\right)\) is:
1. | 3.4 | 2. | 3.6 |
3. | 3.9 | 4. | 3.0 |
Among the following solvents, silver chloride is most soluble in:
1. solution
2. solution
3.
4. Aqueous ammonia
The mixture that will produce a buffer solution when mixed in equal volumes is:
1. | 0.1 mol dm-3 NH4OH and 0.1 mol dm-3 HCl |
2. | 0.05 mol dm-3 NH4OH and 0.1 mol dm-3 HCl |
3. | 0.1 mol dm-3 NH4OH and 0.05 mol dm-3 HCl |
4. | 0.1 mol dm-3 CH3COONa and 0.1 mol dm-3 NaOH |