Question

Need Help ASAP Please! The Answer Needs To Be Numerical

A student ran the following reaction in the laboratory at 546 K:

COCl2 (g) CO (g) + Cl2 (g)

When she introduced 0.723 moles of COCl2 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl2 (g) to be 3.38×10-2 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc =

Answer 1

This problem is providing an equilirium reaction with the initial concentration of COCl2 and the equilibrium concentration of Cl2 for us to calculate the equilibrium constant. At the end, the result is 0.00166.

Chemical equilibrium

In chemistry, not all chemical reactions turn out into completion yet reach a point of constant concentrations (conversion) called equilibrium. In such a way, since this problem is based on this phenomenom, we can start by setting up the equilibrium expression:

$Kc=\frac{[CO][Cl_2]}{[COCl_2]}$

Where each concentration is at equilibrium. Now, since all these species are in 1:1 mole ratio, we can see that the cocentration that changed up to equilibrium is 3.38×10⁻² M (Cl2's concentration), and thus we can calculate Kc with:

$Kc=\frac{(3.38x10^{-2}M)(3.38x10^{-2}M)}{(0.723M-3.38x10^{-2}M)}\\\\Kc=0.00166$

Learn more about chemical equilibrium: https://brainly.com/question/26453983