Respuesta :
Answer : The value of [tex]K_c[/tex] for the following reaction will be, 1024
Explanation :
[tex]K_c[/tex] is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants
The given balanced equilibrium reaction is,
[tex]P_4O_{10}(s)\rightleftharpoons P_4(s)+5O_2(g)[/tex]
As we know that the concentrations of pure solids are constant that means they do not change. Thus, they are not included in the equilibrium expression.
The expression for equilibrium constant for this reaction will be,
[tex]K_c=[O_2]^5[/tex]
Now put all the given values in this expression, we get :
[tex]K_c=(4.000)^5[/tex]
[tex]K_c=1024[/tex]
Therefore, the value of [tex]K_c[/tex] for the following reaction will be, 1024
The value of the equilibrium constant for the given reaction is 1,024.
How we calculate the equilibrium constant?
Equilibrium constant of any chemical reaction at the equilibrium state is calculated as:
Equilibrium constant Kc = Concentration of product / Concentration of reactant
Given chemical reaction is:
P₄O₁₀(s) → P₄(s) + 5O₂(g)
Equilibrium constant for the above reaction is written as:
Kc = [P₄][O₂]⁵ / [P₄O₁₀]
For this reaction only concentration of oxygen gas is taken into consideration, as all other quantities are present in solid form and their value at equilibrium is 1. So, value of Kc is calculated as:
Kc = [O₂]⁵
Given concentration of O₂ = 4M
Kc = (4)⁵ = 1,024
Hence, 1,024 is the value of Kc.
To know more about Equilibrium constant, visit the below link:
https://brainly.com/question/12270624
