The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K.
[N
2] = 1.5 × 10–2M. [H2] = 3.0 ×10–2 M and
[NH
3] = 1.2 ×10–2M.
The equilibrium constant value is:

 1 3.55 × 102 2 20.6 × 103 3 2.06 × 104 4 10.6 × 104
Subtopic:  Introduction To Equilibrium |
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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 Kc for the reaction given below is:

N2(g) + O2(g) $⇋$ 2NO(g)

1. 0.622

2. 6.22

3. 0.562

4. 0.662

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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 Kc for the reaction, PCl5 $⇋$PCl3 + Cl2 is:

1. 0.179

2. 17.9

3. 1.79

4. 179

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

CO(g) + H2O(g) 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

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The value of Kp for the reaction,

CO2 (g) + C (s) $⇋$2CO (g)

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

 1 0.56 bar; 0.15 bar 2 0.15 bar; 0.75 bar 3 0.66 bar; 0.15 bar 4 0.66 bar; 0.25 bar
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The value of Kc for the reaction 2A $⇋$B + C is 2 × 10–3. At a given time, the composition of the reaction mixture is [A] = [B] = [C] = 3 × 104 M.
The reaction will proceed:

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

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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: Kc= 1.80)

1. [PCl
5] = 1.41 M; [PCl3] = [Cl2] = 1.59 M
2. [PCl
5] = 1.61 M; [PCl3] = [Cl2] = 1.59 M
3. [PCl
5] = 1.91 M; [PCl3] = [Cl2] = 1.71 M
4. [PCl
5] = 2.41 M; [PCl3] = [Cl2] = 1.19 M

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