They gave the rxn at Equib as follows

2A (g) + B (g) <====> 2C (g)

0.50 atm of A and 0.20 atm of B are placed in a flask at 300K. At Equib the total pressure is found to be 0.60atm. Calculate the Kp for the reaction.

A. 15.0

B. 4.4

C. 6.6

D. 8.1

E. 1.0 x 10^-4

I dont understand why they used the ICE method.

Answer is B.

I did it by assuming that mole fraction of A is 2/5 and calculating the PP by multiplying 2/4 with 0.6

then for B by calculation mole fraction of B is 1/5 and multiplying that to 0.60

finall mole fraction of C is 2/5 and multiplying that to 0.6

then putting each of these partial pressures in the Equation

K = ( [C]^ 2/[A]^2

**)**

Why am I wrong??

Why am I wrong??