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
Choose the correct option:
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)
Which of the following acids forms three series of salts?
1. | H3PO2 | 2. | H3BO3 |
3. | H3PO4 | 4. | H3PO3 |
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 |
1. solution
2. solution
3.
4. Aqueous ammonia