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Sagot :
The equilibrium constant of a reaction, [tex]K_{c}[/tex] = 6.44 * 10⁵; option C.
What is equilibrium constant of a reaction?
Equilibrium constant, [tex]K_{c}[/tex] of a reaction is a measure of the ratio of the equilibrium concentration of the products of a reaction, to the equilibrium concentration of the reactants; with each concentration raised to the exponent corresponding to the coefficient in the balanced equation of the reaction.
[tex]K_{c} = \frac{(products)^{a}}{(reactants)^{b}}[/tex]
The balanced equation of the given reaction is as follows:
- 2 NO (g) + O₂ (g) ⇄ 2 NO₂ (g)
The concentrations at equilibrium of the species are as follows:
[NO] = 0.0542 M,
[O₂] = 0.127 M, and
[NO₂] = 15.5 M
Equilibrium constant, [tex]K_{c}[/tex] = (15.5)²/(0.127) * (0.0542)²
[tex]K_{c}[/tex] = 6.44 * 10⁵
In conclusion, the equilibrium constant of a reaction, tells on in which direction, the reaction is favored at equilibrium.
Learn more about equilibrium constant at: https://brainly.com/question/12270624
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