The reaction below has an equilibrium constant kp=2.2*106 at 298 k. 2cof2 (g) ⇌co2 (g) + cf4 (g) calculate kp for the reaction below. cof2 (g) ⇌12co2 (g) + 12cf4 (g)

I believe the correct 2nd reaction is:

cof2 (g) ⇌1/2 co2 (g) + 1/2 cf4 (g)

where we can see that it is exactly one-half of the original

Therefore the new Kp is:

new Kp = (old Kp) ^ (1/2)

new Kp = (2.2 x 10^6) ^ (1/2)

new Kp = 1,483.24