In a reaction:A+B < - > 2C When equilibrium was attained, the concentration was [A] = [B] = 4 moles/dm3[C]= 6 moles/dm3The equilibrium constant Kc of this reaction is:
Correct answer: B. 2.25
- A. 1.25
- B. 2.25
- C. 3.25
- D. 2.75
- E. 3.75
Explanation
The equilibrium constant Kc is calculated using the expression: Kc = [C]² / [A][B]. For the reaction A + B < - > 2C, substitute the equilibrium concentrations: [C] = 6 moles/dm3, [A] = [B] = 4 moles/dm3. Thus, Kc = (6)² / (4)(4) = 36 / 16 = 2.25, confirming Option B as correct. Options A, C, D, and E result from errors in calculation or misinterpretation of the equilibrium constant formula.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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