Answer:
<em>a.) What is the equilibrium concentration of CO at 1000 K? : </em><u><em>0.0130M</em></u>
<em>b.) What is the equilibrium concentration of Cl₂ at 1000 K?: </em><u><em>0.0410M</em></u>
<em>c.) What is the equilibrium concentration of COCl₂ at 1000 K?: </em><u><em>0.136M</em></u>
Explanation:
The complete question is:
- <em>Kc= 255 at 1000K for reaction CO(g) + Cl₂(g) ⇄ COCl₂(g). If a mixture initially contains a CO concentration of 0.1490M and a Cl₂ concentration of 0.177M at 1000K, what are the equilibrium concentration of CO, Cl₂ and COCl₂ at 1000K?</em>
<em> a.) What is the equilibrium concentration of CO at 1000 K?</em>
<em> b.) What is the equilibrium concentration of Cl₂ at 1000 K?</em>
<em> c.) What is the equilibrium concentration of COCl₂ at 1000 K?</em>
<h2><em>Solution</em></h2>
<u>1. Write the equilibrium equation</u>
<em> CO(g) + Cl₂(g) ⇄ COCl₂(g)</em>
<u>2. Build the ICE table (initial, change, equilibrium) table</u>
Molar concentrations:
<em> CO(g) + Cl₂(g) ⇄ COCl₂(g)</em>
I 0.1490 0.177 0
C -x -x +x
E 0.01490 - x 0.177 - x x
<u>3. Write the equation of the constant of equilibrium</u>
<u>4. Solve the equation</u>
Use the quadratic equation to obtain:
It cannot be greater than 0.1490, thus the correct solution is 0.136
And the concentrations are:
<em>a.) Concentration of CO: 0.1490M - 0.136M = 0.0130M</em>
<em>b.) Concentration of Cl₂: 0.177M - 0.136M = 0.0410M</em>
<em>c.) Concentration of COCl₂: 0.136M</em>