In which of the following reactions, will the equilibrium mixture contain an appreciable concentration of both reactants and products?

C l_{2} (g) ⇋ 2 C l (g), K_{c} = 6.4 \times 10^{- 39}

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C l_{2} (g) + 2 N O (g) ⇋ 2 N O C l (g), K_{c} = 3.7 \times 10^{8}

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C l_{2} (g) + 2 N O_{2} (g) ⇋ 2 N O_{2} C l (g), K_{c} = 1.8

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H_{2} (g) + S (s) ⇋ H_{2} S (g), K = 7.8 \times 10^{5}

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Solution

The correct option is C $C l_{2} (g) + 2 N O_{2} (g) ⇋ 2 N O_{2} C l (g), K_{c} = 1.8$
The relative proportion of the reactants and products depends upon the value of the equilibrium constants.
Reactions with very high values of equilibrium constants predominately contain products whereas reactions with very low values of equilibrium constants predominately contain reactants.
When the value of the equilibrium constant is of the magnitude of 1, both reactants and products are present in significant quantities.
This is true for the reaction in option C i.e., $C l_{2} (g) + 2 N O_{2} (g) ⇋ 2 N O_{2} C l (g), K_{c} = 1.8$ .

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Similar questions

Q. For which of the following reactions the equilibrium mixture will contain an appreciable concentration of both reactants and products.
(a)

C l_{2} (g) ⇌ 2 C l (g); K_{c} = 6.4 \times 10^{39}

(b)

C l_{2} (g) + 2 N O (g) ⇌ 2 N O C l (g); K_{c} = 3.7 \times 10^{8}

(c)

C l_{2} (g) + 2 N O_{2} (g) ⇌ 2 N O_{2} C l (g); K_{c} = 1.8

Q. Predict which of the following reaction will have appreciable concentration of reactants and products:
a)

{C l}_{2} (g) ⇌ 2 C l (g); K_{c} = 5 \times 10^{- 39}

{C l}_{2} (g) + 2 N O (g) ⇌ 2 N O C l (g); K_{c} = 3.7 \times 10^{8}

{C l}_{2} (g) + 2 {N O}_{2} (g) ⇌ 2 {N O}_{2} C l (g); K_{c} = 1.8

Predict which of the following reaction will have appreciable concentration of reactants and products:

Predict which of the following reaction will have appreciable concentration of reactants and products:
a) $C l_{2} (g) \leftrightarrow 2 C l (g); K_{c} = 5 \times 10^{- 39}$
b) $C l_{2} (g) + 2 N O (g) \leftrightarrow 2 N O C l (g); K_{c} = 3.7 \times 10^{8}$
c) $C l_{2} (g) + 2 N O_{2} (g) \leftrightarrow 2 N O_{2} C l (g); K_{c} = 1.8$

Q. What is the equilibrium constant

K_{c}

for the following reaction at

400 K

2 N O C l (g) ⇌ 2 N O (g) + {C l}_{2} (g)

Δ H^{o} = 77.2 k J, Δ S^{o} = 122 J K^{- 1}

400 K

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