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Given the reaction between 2 gases represented by A2 and B2 to give the compound AB(g). A2(g) + B2(g) ⇌ 2AB(g). At equilibrium, the concentration of A2 = 3.0 × 10^-3 M, of B2 = 4.2 × 10^-3 M, and of AB = 2.8 × 10^-3 M. If the reaction takes place in a sealed vessel at 527°C, then the value of Kc will be:

1. 2.0
2. 1.9
3. 0.62
4. 4.5

Correct answer: 1.9

Solution

The equilibrium constant Kc is calculated using the expression Kc = [AB]^2 / ([A2][B2]). Substituting the given concentrations: Kc = (2.8 × 10^-3)^2 / (3.0 × 10^-3 × 4.2 × 10^-3) = 1.9. Thus, the correct answer is B.

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