We’re being asked to determine the equilibrium constant at 458 ˚C for this reaction:
1/2 Br2(g) ⇌ Br(g)
Given another reaction with it's Kp
Br2(g) ⇌ 2 Br(g) is 3,498
Recall that the equilibrium constant is the ratio of the products and reactants.
We use Kp when dealing with pressure and Kc when dealing with concentration:
Note that solid and liquid compounds are ignored in the equilibrium expression.
At a certain temperature, Kp for the reaction,
Br2(g) <=> 2 Br(g) is 3,498.
Calculate the value of Kp for the reaction,
1/2 Br2(g) ) <=> Br(g)