Question

At a given temperature, the elementary reaction A − ⇀ ↽ − B , in the forward direction, is first order in A with a rate constant of 0.0340 s − 1 . The reverse reaction is first order in B and the rate constant is 0.0740 s − 1 . What is the value of the equilibrium constant for the reaction A − ⇀ ↽ − B at this temperature?

Answer 1

Answer:

0.4595 is the value of the equilibrium constant for the reaction.

Explanation:

A ⇆ B

The forward direction, is first order in A with a rate constant = K =$0.0340 s^{-1}$

The rate of forward reaction = R

$R=K[A]$

The backward direction, is first order in A with a rate constant = K' = $0.0740 s^{-1}$

The rate of backward reaction = R'

$R'=K'[B]$

At equilibrium rate of forward reaction are equal to the rate of backward reaction.

R = R'

$K[A]=K'[B]$

$K_{eq}=\frac{[B]}{[A]}=\frac{K}{K'}=\frac{0.0340 s^{-1}}{0.0740 s^{-1}}=0.4595$

0.4595 is the value of the equilibrium constant for the reaction.