Respuesta :
Answer:
[tex] K = \frac {[Cr_{2}O_{7}^{2-}]}{[CrO_{4}^{2-}]^{2} \cdot [H_{3}O^{+}]^{2}} [/tex]
Explanation:
The equilibrium constant for a given reversible aqueous reaction is defined by the product ratio of the concentrations between the products and reactants:
aA + bB ⇄ cC + dD
[tex] K = \frac {[products]^{p}}{[reactants]^{r}} = \frac {[C]^{c} \cdot [D]^{d}}{[A]^{a} \cdot [B]^{b}} [/tex]
where K: is the equilibrium constant, [C] and [D]: are the product concentrations, [A] and [B]: are the reactant concentrations and a,b,c,d: are the stoichiometric coefficients from the reaction.
Therefore, based on the definition the equilibrium constant of our reaction is:
2CrO₄²⁻(aq) + 2H₃O⁺(aq) ⇄ Cr₂O₇²⁻(aq) + 3H₂O(l)
[tex] K = \frac {[Cr_{2}O_{7}^{2-}]}{[CrO_{4}^{2-}]^{2} \cdot [H_{3}O^{+}]^{2}} [/tex]
Generally, the water concentration is omitted from the expressions.
I hope it helps you!
The equation of the equilibrium constant is; K = [Cr2O7^2−] [H2O]/ [Cr2O7^2−]^2 [H^+]^2.
What is equilibrium constant?
The term equilibrium constant is a value that shows the extent to which reactants are converted into products in a a given reaction.
Now, we have the reaction; 2CrO4 2−(aq)+2H+(aq)⇌Cr2O7 2−(aq)+H2O(l), we can write the equilibrium constant as follows;
K = [Cr2O7^2−] [H2O]/ [Cr2O7^2−]^2 [H^+]^2.
Learn more about equilibrium constant:https://brainly.com/question/17960050