At a given temperature, 2.6 atm of h2 and 3.14 atm of cl2 are mixed and allowed to come to equilibrium. the equilibrium pressure of hcl is found to be 1.13 atm. calculate kp for the reaction at this temperature.

The solution would be like this for this specific problem:

Given:

H2 = 2.6 atm
CL2 = 3.14 atm

 

pressure H2 = 2.6 - x 
pressure Cl2 = 3.14 - x 
pressure HBr = 2x = 1.13

x = 1.13 / 2 = 0.565 

pressure H2 = 2.6 - 0.565 = 2.035
pressure Br2 = 3.14 - 0.565 = 2.575 

Kp = (1.13)^2 / 2.035 x 2.575

 

= 1.2769 / (5.240125)

= 0.24367739319195629875241525726963

= 0.244

Therefore, the Kp for the reaction at the given temperature is 0.244.

To add, the hypothetical pressure of a gas if it alone occupied the whole volume of the original mixture at the same temperature is called the partial pressure or Kp.

Rn in the right answer

There is no reason to think the results are biased or not conducted properly but you should not assume the results are correct just because they were done in a laboratory so the answer would be c. it is likely to be reliable because the results support the conclusion presented.