The reaction of bromine gas with chlorine gas,Br₂(g) + Cl₂(g) $\leftrightarrows$
2 BrCl(g) ,has a K_p value of 7.20.If the initial partial pressures of Br₂,Cl₂,and BrCl in a closed container are all 0.500 atm,what is the equilibrium partial pressure of BrCl(g) ?

Question

The reaction of bromine gas with chlorine gas,Br₂(g) + Cl₂(g)

\leftrightarrows

2 BrCl(g) ,has a K_p value of 7.20.If the initial partial pressures of Br₂,Cl₂,and BrCl in a closed container are all 0.500 atm,what is the equilibrium partial pressure of BrCl(g) ?

Quizplus · Accepted Answer

First, write the equilibrium constant expression and plug in the given values: K_p = [BrCl]2 / ([Br2][Cl2]) K_p = ([x]2) / ([0.500][0.500]) 7.20 = x2 / 0.25 x2 = 1.80 x = 1.34 So the equilibrium partial pressure of BrCl is 1.34 atm, but we need to subtract off the initial pressure of BrCl (which is 0 atm because it is not initially present). Equilibrium partial pressure of BrCl = 1.34 atm - 0.5 atm (initial pressure) = 0.84 atm Therefore, the best choice is D, 0.859 atm, which is the closest to 0.84 atm.

The Reaction of Bromine Gas with Chlorine Gas,Br2(g)+ Cl2(g) ⇆\leftrightarrows⇆ 2 BrCl(g),has a Kp Value of 7

The Reaction of Bromine Gas with Chlorine Gas,Br₂(g)+ Cl₂(g) $\leftrightarrows$ 2 BrCl(g),has a K_p Value of 7