Question

The equilibrium constant K_c for the reaction of hydrogen with iodine is 54.0 at 700 K.

K_c = 54.0 at 700 K

If k_f is the rate constant for the formation of HI and k_r is the rate constant for the decomposition of HI, deduce whether k_r is larger or smaller than k_r

ii. If the value of k_r at 700 K is 1.16 × 10^-3 , what is the value of k_f ?

Answer 1

Given: i. K_c = 54.0 at 700 K

ii. k_r = 1.16 × 10^-3 at 700 K

To find: i. Whether k_f is larger or smaller than k_r

ii. Value of k_f

Formula : K_c = \(\frac{K_f}{K_r}\)

Calculation: 

i. As K_c = \(\frac{K_f}{K_r}\) = 54.0

K_f is greater than k_r by a factor of 54.0.

ii. K_f = K_c x K_r = 54.0 x (1.16 x 10^-3)

= 62.64 x 10^-3

i. K_f is greater than K_r,

ii. Value of K_r is 62.64 x 10^-3