Respuesta :
Answer:
Keq = [O2]³
Explanation:
Step 1: Data given
For the reaction aA + bB ⇄ cC + dD
The Keq is [C]^c * [D]^d / [A]^a * [B]^b
Step 2: The balanced equation
2KClO3(s) ⇔ 2KCl(s) + 3O2(g)
For 2 moles KClO3 we have 2 moles KCl and 3 moles O2
Step 3: Calculate Keq for this reaction
For the reaction aA ⇄ cC + dD
The Keq is [C]^c * [D]^d / [A]^a
Pure solids and liquids are not included in the equilibrium constant expression. This is because they do not affect the reactant amount at equilibrium in the reaction, so they are disregarded and kept at 1. Remember that the activity, a, of any solid or liquid in a reaction is equal to 1
The correct answer here is: Keq = [O2]³
But since it is not an option i would opt for option D, which is the closest to correct.
Keq = [KCl]² *[O2]³ / [KClO3]²
but technically it's not correct. If there is an option 'none of the above' it would be better.
The expression for the equilibrium constant Keq is [KCl]² [O2]³ / [KClO3]²
Finding the equilibrium constant:
The given reaction is as follows:
2KClO₃(s) ⇔ 2KCl(s) + 3O₂(g)
It means that 2 moles KClO₃ produces 2 moles KCl and 3 moles O₂
For a reaction aA ⇄ cC + dD
The Keq is [tex](C)^c (D)^d / (A)^a[/tex]
Pure solids and liquids are not included in the equilibrium constant expression because they do not affect the amount of the reactant at the equilibrium. The activity of any solid or liquid in a reaction is equal to 1.
But here according to the given option and the general expression for the equilibrium constant:
Keq = [KCl]² [O2]³ / [KClO3]²
Learn more about the equilibrium constant:
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