When each of the following processes reach equilibrium, does the system in question contain mostly reactants, mostly products, or fairly equal concentrations of both reactants and products? Justify your answers.

a. 2 H2 (g) + 02 (g) 2 H20 (g)

b. H2 (g + Br2 (g) 2HBr (g) K. 91 x 1080 at 25°C K-114 x 1021 at 25°C

Question

Josephine Moses

Chemistry

21 November, 03:14

When each of the following processes reach equilibrium, does the system in question contain mostly reactants, mostly products, or fairly equal concentrations of both reactants and products? Justify your answers.

a. 2 H2 (g) + 02 (g) 2 H20 (g)

b. H2 (g + Br2 (g) 2HBr (g) K. 91 x 1080 at 25°C K-114 x 1021 at 25°C

+2

Answers (1)

Know the Answer?

Mollie Macdonald · Answer 1

Mostly products

Explanation:

Given the very large equilibrium constants for the two reactions we can consider them to be essentially 100 % complete to the product side.

The equilibrium constant for the reactions are given by:

a. K = p H₂O ² / (p H₂ ² x p O₂) where p are the pressures K = 91 x 10⁸⁰

b. K = p HBr ² / (p H₂ x p Br₂) K = 114 x 10²¹

These two number are so big that essentially very, very little amount of reactants are present after reaction.