Question

Consider the following reaction: COCl2(g) ⇌CO(g) + Cl2(g) Kc = 7.3x10-4 Calculate [CO]eq, [Cl2eq], and [COCl2]eq, respectully, if [COCl2]init=0.730M Group of answer choices no correct answer 0.0216; 0.0216; 0.708 0.229; 0.229; 0.501 0.0416; 0.0416; 0.688 0.0229; 0.0229; 0.707

Answer 1

The concentration of CO at Equilibrium is 0.0361 M

What is Equilibrium Concentration ?

It is a state of dynamic equilibrium where the ratio of the product and reactant concentrations is constant.

Given ;

• Kc = 8.33 x 10⁻⁴
• Molarity of COCl₂ = 1.6 M

Balanced equation ;

• COCl₂ (g) ⇌ CO (g) + Cl₂ (g)

Now, let's calculate final concentrations ;

• Initial concentration of COCl₂ = 1.6M
• Initial concentration of CO and Cl₂ = 0M

There will react X M of COCl₂

Since, the mole ratio is 1 : 1

• Final concentration of CO and Cl₂ will be X M
• Final concentration of COCl₂ will be (1.6 - X) M

Now, Let's find Kc

Kc=  [CO] x [Cl₂] /  [COCl₂]  = 8.33 x 10⁻⁴

Kc = [X] x [X] / 1.6 - X = 8.33 x 10⁻⁴

8.33 x 10⁻⁴  = X² / (1.6 - X)

8.33 x 10⁻⁴ x (1.6 - X) = X²

0.0013328 - 8.33x 10⁻⁴ X = X²

X² + 8.33*10⁻⁴ X  - 0.0013328= 0

X = 0.0361 M = [CO] = [Cl₂]

[COCl₂] = 1.6 - 0.0361 = 1.5639 M

To balance this, we can calculate the Kc

Kc = (0.0361 x 0.0361) / 1.5639 = 0.000833

Learn more about Chemical Equilibrium here ;

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