Answer:
The equilibrium concentration of CO is 0.0361 M
Explanation:
Step 1: Data given
Kc = 8.33 *10^-4
Molarity of COCl2 = 1.6 M
Step 2: The balanced equation:
COCl2(g) ⇌ CO(g) + Cl2(g)
Step 3: Calculate final concentrations
The initial concentration of COCl2 = 1.6M
The initial concentration of CO and Cl2 = 0M
There will react xM of COCl2
Since the mole ratio is 1:1
The final concentration of CO and Cl2 will be X M
The final concentration of COCl2 will be (1.6 -X)M
Step 4: Define Kc
Kc= [CO] *[Cl2] / [COCl2] = 8.33*10^-4
Kc = X*X / 1.6-X = 8.33 * 10^-4
8.33 * 10^-4 = X² /(1.6-X)
8.33 * 10^-4 *(1.6 -X) = X²
0.0013328 - 8.33*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 control this we can calculate the Kc
(0.0361*0.0361)/1.5639 = 0.000833
