The molecule that cannot function as both Bronsted acid and base:
1.
2.
3. HCl
4.
The solubility of in 0.1 M NaOH is:
Ksp ()= 2x
1. 2 x M.
2. 1 x M
3. 1 x M
4. 2 x
At a certain temperature and pressure of 105 Pa, iodine vapour contains 40% by volume of I atoms. The Kp for the equilibrium of the reaction would be:
1. 2.67 104 Pa
2. 1.00 105 Pa
3. 3.63 104 Pa
4. 2.18 105 Pa
Given the reaction 2HI (g) H2 (g) + I2 (g)
A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium, the partial pressure of HI(g) is 0.04 atm. The for the given equilibrium would be:
1. | 2.0 | 2. | 3.5 |
3. | 4.0 | 4. | 2.6 |
A mixture of 1.57 mol of N2, 1.92 mol of H2, and 8.13 mol of NH3 is introduced into a 20 L vessel at 500 K. At this temperature, the equilibrium constant, Kc for the reaction N2 (g) + 3H2 (g) 2NH3 (g) is 1.7 × 102.
The direction of the net reaction is:
1. Reaction is at equilibrium.
2. Reaction will proceed in forwarding direction.
3. Reaction will proceed in the backward direction.
4. Data is not sufficient.
Given the reaction:
2BrCl (g) Br2 (g) + Cl2 (g); Kc= 32 at 500 K. If the initial concentration of BrCl is 3.3 × 10-3 mol L–1, the molar concentration of BrCl in the mixture at equilibrium would be:
1. 3.0 10-2 molL-1
2. 2.0 10-4 molL-1
3. 2.5 10-6 molL-1
4. 3.0 10-4 molL-1
For the reaction, NO(g) + 1/2O2 (g) ⇌ NO2(g)
∆fG° (NO2) = 52.0 kJ/mol , ∆fG° (NO) = 87.0 kJ/mol and
∆fG° (O2) = 0 kJ/mol. The equilibrium constant for the formation of NO2 from NO and O2 at 298K would be:
1. | 2.36 104 | 2. | 3.10 107 |
3. | 1.36 10 | 4. | 2.18 10 |
The equilibrium constant for the following reaction is 1.6 ×105 at 1024K
H2(g) + Br2(g) 2HBr(g)
If HBr at pressure 10.0 bar is introduced into a sealed container at 1024 K, the equilibrium pressure of HBr will be:
1. 11.20 bar
2. 5.56 bar
3. 7.30 bar
4. 9.95 bar
Which of the following is/are the Lewis acids?
(i) BF3 (ii) H2O (iii) H+
1. Only (i)
2. (i) and (ii) only
3. (i), (iii), and (iv) only
4. All of the above
A 0.02 M solution of pyridinium hydrochloride has a pH of 3.44. The ionization constant of pyridine will be:
1. | 2. | ||
3. | 4. |