Consider a chemical reaction 2Cl(g) → Cl2(g) The extent of completing this reaction depends upon the magnitude of Kc and shows that the equilibrium mixture will consist almost of Cl molecules when:
Correct answer: A. Kc is very large
- A. Kc is very large
- B. Kc is very small
- C. Kc is neither very small nor very large
- D. Kc is equal to 1
Explanation
The reaction given is:2Cl(g) \rightleftharpoons Cl_2(g)The equilibrium constant, K_c, is defined as the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients:K_c = \frac{[Cl_2]}{[Cl]^2} * When K_c is very large: This means that the numerator, [Cl_2], is significantly larger than the denominator, [Cl]^2. In other words, at equilibrium, there will be a much higher concentration of Cl_2 molecules compared to Cl atoms. Thus, the equilibrium mixture will consist almost entirely of Cl_2 molecules.
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