Question

What is the relationship between the equilibrium constant (K c ) of reaction and the rate constants for the forward (k) and reverse (k r ) reactions in a single step reaction

Answer 1

Answer: The relationship between the equilibrium constant
`(K_c)` of reaction and the rate constants for the forward
`(k_f)` and reverse
`(k_r)` reactions in a single step reaction is
`K_c=(k_f)/(k_b)`

Step-by-step explanation:

Equilibrium constant is the ratio of product of the concentration of products to the product of concentration of reactants.

For example if the reaction is :
`X\rightleftharpoons Y`

`K_c=([Y])/([X])`

Rate of forward direction=
`k_f[X]`

Rate of backward direction=
`k_b[Y]`

At equilibrium, Rate of forward direction = Rate of backward direction

thus
`(k_f)/(k_b)=(Y)/(X)`

where
`(Y)/(X)=K_c`

Thus
`(k_f)/(k_b)=K_c`