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)

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 =

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.

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

the law of conservation of mass states that in a chemical reaction, the total mass of reactants is equal to the total mass of products. because atoms are only rearranged in a chemical reaction, there must be the same number of sodium atoms and chlorine atoms in both the reactants and products

i do not get it   at all