Question

Find the Keq for this reaction using ICE table?

At a high temperature, 0.50 mol of HBr was placed in a 1.0 L container and allowed to decompose according to the reaction:

2HBr(g) ⇌ H2(g) + Br2(g)

At equilibrium the [Br2] was measured to be 0.13 M. What is Keq for this reaction at this temperature?

Answer 1

Consider,

`2HBr(g) rightleftharpoons H_2(g) + Br_2(g)`

and its ICE table,

where `x = 0.13"M"` (it's given in this problem, which makes it relatively trivial).

Hence,

`K_"eq" = ([Br_2][H_2])/([HBr]^2) = x^2/(0.5-2x)^2 approx 0.123`