Question

Calculate the equilibrium constant for the reaction below given that (CI,] -0.11M, [H,1 -0.15M, and (HCI) - 0.95 M at equilibrium. CI, (e) +H, ()=2 HCI (8)

Answer 1

Answer:

Explanation;

Kc is defined as the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature

Step 1: Write the balanced the chemical equation

Cl₂(g) + H₂(g) <----> 2HCl(g)

Step 2: Extract the data from question

All value at equilibrium is

[Cl₂] = 0.11M

[H₂] = 0.15M

[HCl] = 0.95M

Step 3: Calculate the Kc

Cl₂(g) + H₂(g) <----> 2HCl(g)

Kc = [HCl]² /  × [H₂] × [Cl₂] = (0.95)² /   0.15 × (0.11) = 54.7

Hence the equilibrium constant = 54.7