In the following equilibrium reaction 2A- B-C- the equilibrium concentration of A- B and C are 1- 10 -3 M- 2- 10 -3 M and 3- 10 -3 M respectively at 300 K-Then what is the value of K c for this equilibrium reaction at the same temperature-

The correct option is E 6 The given equillibrium reaction is #160; #160; #160; #160; #160; #160; #160; #160; #160; #160; # ...

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Standard XII

Chemistry

Characteristics of Equilibrium Constant

In the follow...

Question

In the following equilibrium reaction $2 A ⇌ B + C$ , the equilibrium concentration of $A, B$ and $C$ are $1 \times 10^{- 3} M, 2 \times 10^{- 3} M$ and $3 \times 10^{- 3} M$ respectively at $300 K$ .

Then what is the value of $K_{c}$ for this equilibrium reaction at the same temperature?

\frac{1}{6}

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\frac{1}{36}

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\frac{1}{24}

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Solution

The correct option is E $6$
The given equillibrium reaction is
$2 A ⇌ B + C$

Equilibrium constant, $K_{c} = \frac{[B] [C]}{{[A]}^{2}}$
Given, $[A] = 1 \times 10^{- 3} M, [B] = 2 \times 10^{- 3} M, [C] = 3 \times 10^{- 3} M$
By putting all those values, we get

$∴ K_{c} = \frac{(2 \times 10^{- 3}) (3 \times 10^{- 3})}{{(1 \times 10^{- 3})}^{2}} = 6$

Therefore, the correct option is $B$

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

The correct option is E 6The given equillibrium reaction is 2A⇌B+CEquilibrium constant, Kc=[B][C][A]2Given, [A]=1×10−3M,[B]=2×10−3M,[C]=3×10−3MBy putting all those values, we get∴Kc=(2×10−3)(3×10−3)(1×10−3)2=6Therefore, the correct option is B

In the following equilibrium reaction $2 A ⇌ B + C$ , the equilibrium concentration of $A, B$ and $C$ are $1 \times 10^{- 3} M, 2 \times 10^{- 3} M$ and $3 \times 10^{- 3} M$ respectively at $300 K$ .

Then what is the value of $K_{c}$ for this equilibrium reaction at the same temperature?