The following concentrations were obtained for the formation of NH₃ from N₂ and H₂ at equilibrium at 500K.
[N₂] = 1.5 × 10^–2M. [H₂] = 3.0 ×10^–2 M and
[NH₃] = 1.2 ×10^–2M.
The equilibrium constant value is:

At equilibrium, the concentrations of N₂=3.0 × 10^–3M, O₂ = 4.2 × 10^–3M and NO= 2.8 × 10^–3M in a sealed vessel at 800K. The value of K_c for the reaction given below is:

N₂(g) + O₂(g) $\leftrightharpoons$ 2NO(g)

1. 0.622

2. 6.22

3. 0.562

4. 0.662

PCl₅, PCl₃ and Cl₂ are at equilibrium at 500 K and having concentrations 1.59M PCl₃, 1.59M Cl₂ and 1.41 M PCl₅. The value of K_c for the reaction, PCl₅ $\leftrightharpoons$PCl₃ + Cl₂ is:

1. 0.179

2. 17.9

3. 1.79

4. 179

The value of K_c = 4.24 at 800K for the reaction,

CO(g) + H₂O(g) $\leftrightharpoons$CO₂ (g) + H₂ (g)

If only CO and H₂O are present initially at concentrations of 0.10M each.

The equilibrium concentrations of CO₂, and CO are-

1. 0.067 M; 0.033 M
2. 0.76 M; 0.029 M
3. 0.65 M; 0.027 M
4. 0.061 M; 0.30 M

The value of K_p for the reaction,

CO₂ (g) + C (s) $\leftrightharpoons$2CO (g)

is 3.0 at 1000 K. If initially  \(P_{CO_{2}}\)= 0.48 bar and P_CO = 0 bar and pure graphite is present.
The equilibrium partial pressures of CO and CO₂ are respectively-

The value of K_c for the reaction 2A $\leftrightharpoons$B + C is 2 × 10^–3. At a given time, the composition of the reaction mixture is [A] = [B] = [C] = 3 × 10^–4 M.
The reaction will proceed:

1. In the backward direction
2. In the forward direction
3. In both direction
4. Cannot be predicted

3.00 mol of PCl₅ kept in 1L closed reaction vessel was allowed to attain equilibrium at 380K. The
composition of the mixture at equilibrium is:
(Given: K_c= 1.80)

1. [PCl₅] = 1.41 M; [PCl₃] = [Cl₂] = 1.59 M
2. [PCl₅] = 1.61 M; [PCl₃] = [Cl₂] = 1.59 M
3. [PCl₅] = 1.91 M; [PCl₃] = [Cl₂] = 1.71 M
4. [PCl₅] = 2.41 M; [PCl₃] = [Cl₂] = 1.19 M