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.
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To calculate the equilibrium constant (Kp) for the given reaction, you need to use the equation:
Kp = (P(BrCl))^2 / (P(Br2) * P(Cl2))
Given:
P(Br2) = 0.5417 atm
P(Cl2) = 0.6962 atm
P(BrCl) = 0.3442 atm (initial pressure)
However, we need the equilibrium pressure of Cl2(g) in order to calculate Kp correctly. The given value of 0.7246 atm is the equilibrium pressure of Cl2(g).
To find Kp, we will rearrange the equation to solve for Kp:
Kp = (P(BrCl))^2 / (P(Br2) * P(Cl2))
Using the given values:
Kp = (0.3442)^2 / (0.5417 * 0.7246)
Kp = 0.1182 / 0.3933
Kp ≈ 0.3000
Note that the calculated value of Kp is not exactly 0.2000 as you mentioned. Please check the values and equations provided to ensure accuracy.