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Characteristics of Equilibrium Constant

The equilibri...

Question

The equilibrium constant $K_{c}$ of the reaction $2 A ⇌ B + C$ is $0.5$ at $25^{o}$ C and 1 atm. The reaction will proceed in the backward direction when concentrations $[A], [B]$ and $[C]$ are respectively.

A

10^{- 3}, 10^{- 2}

and

10^{- 2}

M

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B

10^{- 1}, 10^{- 2}

and

10^{- 2}

M

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C

10^{- 2}, 10^{- 2}

and

10^{- 3}

M

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D

10^{- 2}, 10^{- 3}

and

10^{- 3}

M

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Solution

The correct option is B $10^{- 3}, 10^{- 2}$ and $10^{- 2}$ M
$Q_{c} = \frac{[B] [C]}{[A]^{2}} = \frac{[10^{- 2}] [10^{- 2}]}{[10^{- 3}]^{2}} = 10^{2} > K_{c}$

Hence, the reaction will move in backward direction.

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Similar questions

Q. In the following equilibrium reaction

2 A ⇌ B + C

, the equilibrium concentration of

A, B

C

1 \times 10^{- 3} M, 2 \times 10^{- 3} M

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?

Q. The value of

k_{c}

for the reaction

2 A ⇌ B + C

10^{- 3}

At a given time the composition of reaction mixture is [A] = [B] = [C] = 3 x

10^{- 4}

M. In which direction the reaction will proceed?

Q. For the reaction

A + B \to C

; starting with different initial concentrations of A and B, the initial rate of reaction were determined graphically in four experiments. Find the rate of reaction (

r

S.No.	[A] M (Initial conc.)	[B] M (Initial conc.)	rate (M $s e c^{- 1}$ )
1	$1.6 \times 10^{- 3}$	$5 \times 10^{- 2}$	$10^{- 3}$
2	$3.2 \times 10^{- 3}$	$5 \times 10^{- 2}$	$4 \times 10^{- 3}$
3	$1.6 \times 10^{- 3}$	$10^{- 1}$	$2 \times 10^{- 3}$
4	$3.2 \times 10^{- 3}$	$10^{- 1}$	$8 \times 10^{- 3}$

Q. Consider the following reaction and its equilibrium constant:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g) K c = 5.85 \times 10^{- 3}

A reaction mixture at a particular time, t contains:

[N O_{2}] = 0.025 M a n d [N_{2} O_{4}] = 0.033 M .

Q c

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The following are the data for the reaction

A + B \to

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(m o l L^{- 1} s^{- 1})

(i) 0.1 M 0.1 M

4.0 \times 10^{- 4}

(ii) 0.2 M 0.2 M

1.6 \times 10^{- 3}

(iii) 0.5 M 0.1 M

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(iv) 0.5 M 0.5 M

1.0 \times 10^{- 2}

The reaction rate when the concentration of A and B are 0.4 M and 0.7 M respectively :

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