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2 years ago

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Which of the following equilibrium expressions corresponds to a heterogeneous equilibrium?(a) Kc =[NH4+][OH−][NH3](b) Kc =[H+][C

2H3O2−][HC2H3O2](c) Kc =[Ag(NH3)2+][Cl−][NH3]2(d) Kc = [Ba2+][F−]2

1 answer:

Alex777 [14]2 years ago

6 0

Answer:

c. $Kc = \frac{[Ag(NH_{3})_2^{+}][Cl^-]}{[NH_3]^2}}$

d. $Kc = [Ba^{2+}][F^{-}]^2$

Explanation:

An heterogeneous equilibrium is defined as a system whose reactants, products, or both are in more than one phase.

Also, you must know in an equilibrium constant you don't take solids or pure liquids. Thus:

a. $Kc = \frac{[NH_{4}^+][OH^-]}{[NH_3]}}$

The reaction must be: NH₃(aq) + H₂O(l) ⇆ NH₄⁺(aq) + OH⁻(aq) <em>All reactants are in the same phase.</em>

b. $Kc = \frac{[H^+][C_2H_3O_{2}^-]}{[HC_2H_3O_2]}}$

The reaction must be: HC₂H₃O₂(aq) ⇄ H⁺(aq) + C₂H₃O₂⁻(aq) <em>All reactants are in the same phase.</em>

c. $Kc = \frac{[Ag(NH_{3})_2^{+}][Cl^-]}{[NH_3]^2}}$

The reaction must be: 2NH₃(aq) + AgCl(s) ⇄ Ag(NH₃)₂⁺(aq) + Cl⁻(aq)

<em>Reactants aren´t in the same phase. Heterogeneous equilibrium</em>

d. $Kc = [Ba^{2+}][F^{-}]^2$

The reaction must be: BaF₂(s) ⇆ Ba²⁺(aq) + 2F⁻(aq)

<em>Reactants aren´t in the same phase. Heterogeneous equilibrium</em>

I hope it helps!

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