Assume that the change in concentration of COCl2 is small enough to be neglected in the following problem. Use an ICE table with the "x is small" approximation. The results might surprise you. You can trust them if you verify the assumption. (a) Calculate the equilibrium concentration of all species in an equilibrium mixture that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g) + Cl2(g) Kc=2.200 × 10−10 Enter the equilibrium molar concentration of COCl2 below, with 4 sig figs
Assume that the change in concentration of COCl2 is small enough to be neglected in the following problem. Use an ICE table with the "x is small" approximation. The results might surprise you. You can trust them if you verify the assumption.
(a) Calculate the equilibrium concentration of all species in an equilibrium mixture that results from the decomposition of COCl2 with an initial concentration of 0.3166 M.
COCl2(g) ⇌ CO(g) + Cl2(g) Kc=2.200 × 10−10
Enter the equilibrium molar concentration of COCl2 below, with 4 sig figs
Given data :
initial concentration of COCl2 = 0.3166 M.
Kc=2.200 × 10-10
Chemical equation :
COCl2(g) ⇌ CO(g) + Cl2 (g)
To find : Equilibrium molar concentration of COCl2
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