Respuesta :
Answer:
For a: The equilibrium mixture contains primarily reactants.
For b: The equilibrium mixture contains primarily products.
Explanation:
There are 3 conditions:
- When [tex]K_{eq}>1[/tex]; the reaction is product favored.
- When [tex]K_{eq}<1[/tex]; the reaction is reactant favored.
- When [tex]K_{e}=1[/tex]; the reaction is in equilibrium.
For the given chemical reactions:
- For a:
The chemical equation follows:
[tex]HCN(aq.)+H_2O(l)\rightleftharpoons CN^-(aq.)+H_3O^+(aq.);K_{eq}=6.2\times 10^{-10}[/tex]
The expression of [tex]K_{eq}[/tex] for above reaction follows:
[tex]K_{eq}=\frac{[CN^-][H_3O^+]}{[HCN][H_2O]}=6.2\times 10^{-10}[/tex]
As, [tex]K_{eq}<1[/tex], the reaction will be favored on the reactant side.
Hence, the equilibrium mixture contains primarily reactants.
- For b:
The chemical equation follows:
[tex]H_2(g)+Cl_2(g)\rightleftharpoons 2HCl(g);K_{eq}=2.51\times 10^{4}[/tex]
The expression of [tex]K_{eq}[/tex] for above reaction follows:
[tex]K_{eq}=\frac{[HCl]^2}{[H_2][Cl_2]}=2.51\times 10^{4}[/tex]
As, [tex]K_{eq}>1[/tex], the reaction will be favored on the product side.
Hence, the equilibrium mixture contains primarily products.
Based on the equilibrium expression of the reactions;
- reactant formation is favored in part A and the mixture contains primarily reactants since Keq < 1.
- product formation is favored in part B the equilibrium mixture contains primarily products, since Keq > 1.
What is equilibrium constant, K?
The equilibrium constant, K is a ratio that shows the concentrations of the products divided by the concentrations of the reactants.
In determining which side of a reaction is favored at equilibrium;
- When Keq > 1; product formation is favored
- When Keq < 1; reactant formation is favored.
- When Keq = 1 ; the reaction is at equilibrium.
For Part A:
The chemical equation for the equilibrium reaction is as follows:
HC-N(aq) + H₂O(l) ⇄ C-N⁻ (aq) + H₃O⁺ (aq) Keq = 6.2 * 10⁻¹⁰
the equilibrium constant expression is as follows;
Keq = [C-N⁻ ] [H₃O⁺] / [HC-N] [H₂O] = 6.2 * 10⁻¹⁰
Since Keq < 1; reactant formation is favored and the mixture contains primarily reactants.
For Part B:
The chemical equation for the equilibrium reaction is as follows:
H₂(g) + Cl₂(l) ⇄ 2 HCl (g) Keq = 2.51 * 10⁴
the equilibrium constant expression is as follows;
Keq = [HCl ]² / [H₂] [Cl₂] = 2.51 * 10⁴
Since Keq > 1; product formation is favored and the equilibrium mixture contains primarily products.
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