Question

Calculate K for the following reaction:

A + 2 B ⇌ 2 C + D

given the following K values:

A ⇌ D + 2 E K1 = 72.41

C ⇌ B + E K2 = 38.81

Answer 1

Solution.

K1 and K2 equally:

$K1=\dfrac{[D]*[E]^2}{[A]}$ ;

$K2=\dfrac{[B]*[E]}{[C]}$ .

Express K through K1 and K2:

$K= \dfrac{[C]^2*[D]}{[A]*[B]^2}= \dfrac {[C]^2*[D]*[E]^2}{[A]*[B]^2*[E]^2}=\dfrac {[D]*[E]^2}{[A]}*\dfrac {[C]^2} {[B]^2*[E]^2}=K1*​ \Bigg ( { \dfrac {1}{K2}}\Bigg)^2=​ \dfrac{K1}{K2^2}$ .

Calculate K:

$K=​ \dfrac{72.41}{38.81^2}=0.048.$

Answer: 0.048.