In the following equilibrium reaction 2A leftharpoons B + C, the equilibrium concentrations of A, B and C are 1 × 10-3 M 2 × 10-3 M and 3 × 10-3M respectively at 300 K. The value of Kc for this equilibrium at the same temperature is

Question

In the following equilibrium reaction 2A leftharpoons B + C, the equilibrium concentrations of A, B and C are 1 × 10-3 M 2 × 10-3 M and 3 × 10-3M respectively at 300 K. The value of Kc for this equilibrium at the same temperature is (A) (1/6) (B) 6 (C) (1/36) (D) 36

Tardigrade Admin · Accepted Answer

For the reaction, 2 A leftharpoons B+C Equilibrium constant, Kc=([B][C]/[A]2) Given, [A]=1 × 10-3 M , [B]=2 × 10-3 M, [C]=3 × 10-3 M ∴ Kc=((2 × 10-3)(3 × 10-3)/(1 × 10-3)2)=6

Q. In the following equilibrium reaction $2 A ⇌ B + C$ , the equilibrium concentrations of $A, B$ and $C$ are $1 \times 1 0^{- 3} M$ $2 \times 1 0^{- 3} M$ and $3 \times 1 0^{- 3} M$ respectively at $300 K$ . The value of $K_{c}$ for this equilibrium at the same temperature is

$\frac{1}{6}$

$6$

$\frac{1}{36}$

$36$

$\frac{1}{24}$

For the reaction,

$2 A ⇌ B + C$

Equilibrium constant, $K_{c} = \frac{[ B ] [ C ]}{[ A ] ^{2}}$

Given, $[A] = 1 \times 1 0^{- 3} M, [B] = 2 \times 1 0^{- 3} M$ ,

$[C] = 3 \times 1 0^{- 3} M$

$∴ K_{c} = \frac{( 2 \times 1 0 ^{- 3} ) ( 3 \times 1 0 ^{- 3} )}{( 1 \times 1 0 ^{- 3} ) ^{2}} = 6$

Q. In the following equilibrium reaction 2A⇌B+C, the equilibrium concentrations of A,B and C are 1×10−3M 2×10−3M and 3×10−3M respectively at 300K. The value of Kc​ for this equilibrium at the same temperature is

61​

6

361​

36

241​

For the reaction, 2A⇌B+C Equilibrium constant, Kc​=[A]2[B][C]​ Given, [A]=1×10−3M,[B]=2×10−3M, [C]=3×10−3M ∴Kc​=(1×10−3)2(2×10−3)(3×10−3)​=6