Question

If a reaction mixture initially contains a COCO concentration of 0.1490 MM and a Cl2Cl2 concentration of 0.177 MM at 1000 KK. What is the equilibrium concentration of COCO at 1000 KK?

Answer 1

Answer:

a.) What is the equilibrium concentration of CO at 1000 K? : 0.0130M

b.) What is the equilibrium concentration of Cl₂ at 1000 K?: 0.0410M

c.) What is the equilibrium concentration of COCl₂ at 1000 K?: 0.136M

Explanation:

The complete question is:

• 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?

        a.) What is the equilibrium concentration of CO at 1000 K?

        b.) What is the equilibrium concentration of Cl₂ at 1000 K?

        c.) What is the equilibrium concentration of COCl₂ at 1000 K?

Solution

1. Write the equilibrium equation

      CO(g) + Cl₂(g) ⇄ COCl₂(g)

2. Build the ICE table (initial, change, equilibrium) table

Molar concentrations:

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

I                  0.1490                0.177                    0

C                   -x                        -x                      +x

E                 0.01490 - x          0.177 - x              x

3. Write the equation of the constant of equilibrium

         $K_c=\dfrac{[COCl_2]}{[CO][Cl_2}}$

          $255=\dfrac{x}{(0.1490-x)(0.177-x)}$

4. Solve the equation

          $255(0.026373-0.1490x-0.177x+x^2)=x$

         $6.725115-37.995x-45.135x+255x^2=x$

         $255x^2-84.13x+6.725115=0$

Use the quadratic equation to obtain:

• x = 0.136 and x = 0.194

It cannot be greater than 0.1490, thus the correct solution is 0.136

And the concentrations are:

a.) Concentration of CO: 0.1490M - 0.136M = 0.0130M

b.) Concentration of Cl₂: 0.177M - 0.136M = 0.0410M

c.) Concentration of COCl₂: 0.136M