Question

The reaction below has an equilibrium constant Kp=2.2×10^6 at 298K. 2COF2(g)⇌CO2(g)+CF4(g).Calculate Kp for the reaction below. COF2(g)⇌1/2CO2(g)+1/2CF4(g) Express your answer using two significant figures.

Answer 1

Solution :-

2COF2(g)⇌CO2(g)+CF4(g)       kp1= 2.2*10^6

COF2(g)⇌1/2CO2(g)+1/2CF4(g) kp2 =?

The kp value of the original reaction is given and asked to calculate the kp value when the reaction coefficients are halved (half)

When the reaction coefficients are halved or when reaction is divided by 2 then we have to take the square root of the original kp

Therefore kp for the new reaction is calculated as follows

Kp2= kp1

Kp2= [2.2*10^6]

Kp2=1.5*10^3

Therefore the Kp for the final reaction is 1.5*10^3