AIPMT MAINS 2010 Chemistry Equilibrium Constant MCQ Question
The reaction 2A(g) + B(g) ⇌ 3C(g) + D(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression
[(0.75)³(0.25)]/[(1.00)²(0.00)]
[(0.75)³(0.25)]/[(0.50)²(0.75)]
[(0.75)³(0.25)]/[(0.50)²(0.25)]
[(0.75)³(0.25)]/[(0.75)²(0.25)]
Correct Answer
Detailed Explanation
Using the equilibrium expression K = [C]³[D]/[A]²[B], substituting the equilibrium concentrations gives K = [(0.75)³(0.25)]/[(0.50)²(0.75)].
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