Question

Calculate the equilibrium constant for the reaction below given that [Cl2] = 0.21 M, [H2] = 0.13 M, and [HCl] = 0.95 M at equilibrium. Given: Cl2(g) + H2(g) ⇌ 2HCl(g)

Answer 1

Answer:

The equilibrium constant for this reaction is 33

Explanation:

Step 1: Data given

[Cl2] = 0.21 M

[H2] = 0.13 M

[HCl] = 0.95 M

Step 2: The balanced equation

Cl2(g) + H2(g) ⇌ 2HCl(g)

Step 3: Calculate the equilibrium constant

K = [HCl]² / [Cl2][H2]

K = [0.95]² /[0.21][0.13]

K = 33.06 ≈ 33

The equilibrium constant for this reaction is 33

Answer 2

Answer:

The answer to your question is  Ke = 33.06

Explanation:

Data

[Cl₂] = 0.21 M

[H₂] = 0.13 M

[HCl] = 0.95 M

Balanced chemical reaction

                      Cl₂(g)  +  H₂(g)  ⇔  2HCl (g)

Formula

               Ke = $\frac{[HCl]^{2}}{[Cl_{2][H_{2}]}}$

Substitution

               Ke = [0.95]² / [0.21][0.13]

Simplification

              Ke = 0.9025 / 0.0273

Result

              Ke = 33.06

The equilibrium constant does not have units.