Equilibrium · Question 10

At a given temperature and pressure, the equilibrium constant values for the equilibria are given below: 3A2 + B2 2A3B, K1 A3B 32A2 + 12B2, K2 The relation between K1 and K2 is :

1. K12 = 2K2
2. K2 = K12
3. K1 = 1 K2
4. K2 = 1 K1

For the reaction in equilibrium N2(g) + 3H2(g) 2NH3(g), H = -Q Reaction is favoured in forward direction by:

1. use of catalyst
2. decreasing concentration of N2
3. low pressure, high temperature and high concentration of ammonia
4. high pressure, low temperature and higher concentration of H2

The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is: (Given : Solubility product of AgCl = 10-10)

1. 10-4
2. 10-6
3. 10-9
4. 10-5

Amongst the given options which of the following molecules/ion acts as a Lewis acid?

1. H2O
2. BF3
3. OH-
4. NH3

The equilibrium concentrations of the species in the reaction A + B C + D are 2, 3, 10 and 6 mol L-1, respectively at 300 K. G for the reaction is (R = 2 cal/mol K)

1. -137.26 cal
2. -1381.80 cal
3. -13.73 cal
4. 1372.60 cal

For the reaction N2(g) + 3H2(g) 2NH3(g), H = -92.4 kJ mol-1. The yield of ammonia increases on

1. increasing temperature
2. decreasing pressure
3. increasing pressure
4. adding a catalyst

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is [Given pKa of CH3COOH = 4.57]

1. 5.57
2. 3.57
3. 4.57
4. 2.57

3O2(g) 2O3(g) for the above reaction at 298 K, Kc is found to be 3.0 10-59. If the concentration of O2 at equilibrium is 0.040 M then concentration of O3 in M is

1. 4.38 10-32
2. 1.9 10-63
3. 2.4 1031
4. 1.2 1021

0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :

1. 1
2. 3
3. 2
4. 4

Kp for the following reaction is 3.0 at 1000 K. CO2(g) + C(s) 2CO(g) What will be the value of Kc for the reaction at the same temperature? (Given : R = 0.083 L bar K-1 mol-1)

1. 3.6
2. 0.36
3. 3.6 10-2
4. 3.6 10-3