Question

Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) Kc=2.99×10−7 at 227∘C

If a reaction mixture initially contains 0.195 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 ∘C?

Answer 1

SO₂Cl₂(g) <--> SO₂ (g) Cl₂ (g)

Use Initial, Change and Equilibrium Value

[A] <--> [C] [D]
I .195 0 0
C -x +x +x
E .195-x X X

2.99X10-7 = X^2/ (.195-X)
5.83X10-8 - 2.99X10-7 = X^2
A B C
X^2 + 2.99X10-7 - 5.83X10-8 = 0
Take the square root of everything I placed into brackets.

2.99x10-7 + or - {(2.99x10-7)^2-4(1)(-5.83X10-8)} / 2(1)

2.99x10-7 + or - 4.829 X10-4 / 2

X₁ = 2.41 X 10^-4
X₂ = -2.41 X 10^-4

Has to be X1, we can't have a negative value for Molarity.