Answered

At Westonci.ca, we connect you with the answers you need, thanks to our active and informed community. Connect with a community of experts ready to provide precise solutions to your questions on our user-friendly Q&A platform. Get immediate and reliable solutions to your questions from a community of experienced professionals on our platform.

Given the following reaction: 2 NO(g) + O2(g) <--> 2 NO2(g), what is the equilibrium constant (K), if the concentrations at equilibrium are [NO] = 0.0542 M, [O2] = 0.127 M, and [NO2] = 15.5 M?
Group of answer choices

A. K = 2.35 x 102

B. K = 2.54 x 10-1

C. K = 6.44 x 105

D. K = 3.4 x 103

Sagot :

mickymike92

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

#SPJ1

We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Westonci.ca is committed to providing accurate answers. Come back soon for more trustworthy information.