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NEET CHEMISTRYMedium

For the reaction 2A⇌B+C2\text{A} \rightleftharpoons \text{B} + \text{C}; Kc=4×10−3K_c = 4 \times 10^{-3}. At a given time, the composition of the reaction mixture is: [A]=[B]=[C]=2×10−3 M[\text{A}] = [\text{B}] = [\text{C}] = 2 \times 10^{-3}\text{ M}. In light of the above facts, which of the following is correct?

A

Reaction has a tendency to go in the forward direction.

B

Reaction has a tendency to go in the backward direction.

C

Reaction has gone to completion in the forward direction.

D

Reaction is at an equilibrium.

Step-by-Step Solution

For the reaction 2A⇌B+C2\text{A} \rightleftharpoons \text{B} + \text{C}, the reaction quotient (QcQ_c) at the given time is calculated using the expression: Qc=[B][C][A]2Q_c = \frac{[\text{B}][\text{C}]}{[\text{A}]^2}

Substituting the given concentrations ([A]=[B]=[C]=2×10−3 M[\text{A}] = [\text{B}] = [\text{C}] = 2 \times 10^{-3}\text{ M}): Qc=(2×10−3)(2×10−3)(2×10−3)2=1Q_c = \frac{(2 \times 10^{-3})(2 \times 10^{-3})}{(2 \times 10^{-3})^2} = 1

We are given the equilibrium constant Kc=4×10−3K_c = 4 \times 10^{-3} (or 0.0040.004). Comparing QcQ_c and KcK_c, we find that Qc>KcQ_c > K_c (1>0.0041 > 0.004). When the reaction quotient is greater than the equilibrium constant (Qc>KcQ_c > K_c), the reaction will proceed in the reverse (backward) direction to reach equilibrium .

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