Question

For the equilibrium, 2nocl(g)  2no (g) + cl (g), the value of equilibrium constant, kc is 3.75 x 10-6 at 1069 k. calculate kp for the reaction at this temperature

Answer 1

Answer:

Ans = 0.033

Explanation:

As we know, Kp = Kc (RT)^delta 'n'

For the above reaction,

delta 'n' = moles of product - moles of reactant

= {no.of moles of NO(g) + no.of moles of Cl 2(g)} - {no.of moles of NOCl(g)}

= (2+1) - 2 = 1

Kp = 3.75 × 10^-6 (8.31 × 1069)

= 0.033

Hence, Kp = 0.033

( point need to be noted in this question is - value of R , rydberg constant is 8.31 not 0.083 )

Thanks, hope you clear the concept easily

Answer 2

Answer:

answer in attachment..... since the unit of Kc is not given in question i have taken rydberg constant to be 0.08