Question

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M, [HI]eq = 5.6 × 10-16 M, [Cl2]eq = 0.0019 M. 2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g)

Answer 1

3.53*
`10^(-32)`

Step-by-step explanation:

`K_(c) =([HI]^(2)[Cl_(2)] )/([HCl]^(2))=([5.6*10^(-16) ]^(2) [0.0019])/([0.13]^(2) )=3.53*10^(-32)`

Kc is the equilibrium constant calculated as the ration of products over reactants with their stoichiometric coefficients as their exponents. So the balanced chemical equation is important. Solids do not form part of the Kc expression, they do not affect the equilibrium constant which is why Iodine is not part of the calculations