At a certain temperature and pressure of 10⁵ Pa, iodine vapour contains 40% by volume of I atoms. The K_p for the equilibrium of the reaction would be:

 $I_2 \left(g\right) \leftrightharpoons 2I \left(g\right)$

1. 2.67 $\times$ 10⁴ Pa

2. 1.00 $\times$ 10⁵ Pa

3. 3.63 $\times$ 10⁴ Pa

4. 2.18 $\times$ 10⁵ Pa

Given the reaction 2HI _(g) $\rightleftharpoons$ H_2 (g) + I_2 (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 ${\mathrm{K}}_{\mathrm{P}}$ for the given equilibrium would be:

A mixture of 1.57 mol of N₂, 1.92 mol of H_2, and 8.13 mol of NH₃ is introduced into a 20 L vessel at 500 K. At this temperature, the equilibrium constant, K_c for the reaction N_2 (g) + 3H_2 (g) $\rightleftharpoons$ 2NH_3 (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) $\leftrightharpoons$ Br_2 (g) + Cl_2 (g); K_c= 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 $\times$ 10^-2 molL^-1

2. 2.0 $\times$ 10^-4 molL^-1

3. 2.5 $\times$ 10^-6 molL^-1

4. 3.0 $\times$ $$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:

The equilibrium constant for the following reaction is 1.6 ×10⁵ at 1024K

H_2(g) + Br_2(g)  $\leftrightharpoons$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

A 0.02 M solution of pyridinium hydrochloride has a pH of 3.44. The ionization constant of pyridine will be:

The K_sp of Ag₂CrO₄ and AgBr is 1.1 × 10^–12 and 5.0 × 10^–13 respectively.

When equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together (K_{sp  (cupric iodate)} = 7.4 × 10^–8 ), from the following, the correct observation would be :

The minimum volume of water required to dissolve 1g of calcium sulphate at 298 K is

(For CaSO₄ , K_sp is 9.1 × 10^–6)

1. 1.22 L

2. 0.69 L

3. 2.44 L

4. 1.87 L