Question

Consider the reaction: H2 (g) + Br2 (g) ⇆ 2HBr (g

Suppose that the value of the equilibrium constant is very large, which species will predominate at equilibrium?

[1] H2

[2] Br2

[3] HBr

[4] Both H2 and Br2

[5] All species will have the same concentration.

Answer 1

H₂ + Br₂ = 2 HBr

$K_c = \cfrac {[HBr]²}{[H_2][Br_2]}$

According to the above formula Kc, the higher the concentration of the substance formed, the larger Kc. That is HBr

Answer: [3] HBr