The equilibrium constant, kc, for the following reaction is 77.5 at 600 k. co(g) + cl2(g) cocl2(g) calculate the equilibrium concentrations of reactant and products when 0.442 moles of co and 0.442 moles of cl2 are introduced into a 1.00 l vessel at 600 k. [co] = m [cl2] = m [cocl2] = m

     [COCl₂] = 0.373 mol·L⁻¹

[CO] = [Cl₂] = 0.069 mol·L⁻¹

Explanation:

The balanced equation is

CO + Cl₂ ⇌ COCl₂

Data:

      Kc = 77.5

n(CO₂) = 0.442 mol

 n(Cl₂) = 0.442 mol

       V = 1.00 L

1. Calculate the initial concentration of CO and Cl₂

Step 2. Set up an ICE table.

Step 3. Calculate the equilibrium concentrations

[COCl₂] = x mol·L⁻¹ = 0.373 mol·L⁻¹

[CO] = [Cl₂] = (0.442 - 0.373) mol·L⁻¹ = 0.069 mol·L⁻¹

a. hope i'm right

explanation: