For the reversible reaction in equilibrium :

CHEMISTRY · Subjective · A Level · Chemistry · Rate equations · Rate equations

Problem

A \xrightleftharpoons[K_2]{K_1} B

. The values of

K_1

and

K_2

are

2 \times 10^{-3} \text{ mol L}^{-1} \text{ sec}^{-1}

and

3 \times 10^{-3} \text{ sec}^{-1}

respectively. If we add 0.5 moles of

B

in the equilibrium mixture, initially containing 2 moles of

A

. Calculate the time taken for concentration of

B

to become equal to

3/4

of the concentration of

A

at initial equilibrium. The volume of mixture is 1 L and remains constant.