Posted by
**Tracy** on
.

At 389K, this reaction has a Kc value of 0.0682. 2X(g) + 2Y(g) <-> Z(g) .. Calculate Kp at 389K. Kp=

this is what I did.. can somebody confirm or find any mistakes in my thought process?

Kp = Kc(R)(T)^Delta n

Delta n = (1)-(2+2) = -3

Kp = (0.0682)(0.08206)(398K)^-3 = 0.09678

i'm confused because I'm not sure if delta n is allowed to be negative. please help!