The equilibrium constant Kc for the reaction is 3.8 10-5 at 727°C. What are Kc and Kp for the following equilibrium at the same temperature?

2 I (g) <=> I2 (g)

1 Answer
Mar 6, 2018

K_pKp=3.12*10^-33.12103

Explanation:

The relationship between K_cKc and K_pKp is in the formula K_c=K_p*(RT)^(Delta n)
The R value used is in atmospheres and the T value is in kelvins. Delta n is the sum of the coefficients of products minus the sum of the coefficients of the reactants.
Example
aA+bB<=> cC+bB
Delta n = (c+b)-(a+b)
The Delta n for the chemical formula gives is -1 so the product of RT is raised to the -1.
K_c/((RT)^-1)=K_p
(3.8*10^-5)/((.0821* 964.15)^-1)~~3.12*10^-3