The initial pressure for the compounds involved in the reaction shown were determined to be P(Br2(g)) = 0.5417 atm, P(Cl2(g)) = 0.6962 atm, P(BrCl(g)) = 0.3442 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure of Cl2(g) was 0.7246 atm.

Question

The initial pressure for the compounds involved in the reaction shown were determined to be P(Br2(g)) = 0.5417 atm, P(Cl2(g)) = 0.6962 atm, P(BrCl(g)) = 0.3442 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure of Cl2(g)  was 0.7246 atm.

Br2(g)+Cl2(g) = 2BrCl(g)

The answer is 0.2000. I having hard time getting this answer. Thanks.

DrBob222 · Answer

If you are still having trouble with this, please post again at the top of the page and someone will help. It would help if you posted your work and we can find the error.