Ok, I thought that people would not care about my working out, this is my working out:
Before I go on, all my equations are not written in fractions but in divisions. I tried using the LaTeX code \frac{numerator}{denominator} and others but it would not work.
The Kc is 22/(1 × 33) = 4/27
The molarity of each molecule immediately after concentration of A is increased is A = 2 M, B = 3 M and C = 2 M. If x molarity of A is converted into reactants then 3x molarity of B would be converted and C would have an increase of 2x molarity.
So then if we put this into the Kc then:
4/27 = (2+2x)2/((2-x) × (3-3x)3)
x = 0.12 or 3.4
A cannot be decreased by 3.4 so x = 0.12
A = 2 - 0.12 B = 3 - 0.12 × 3 C = 2 + 0.12 × 2
= 1.88 = 2.64 = 2.24
Borek, in your reply, to my equilibrium constant post on equilibrium concentrations from initial concentrations you used a mixture of stoichiometry and relations between the molecules. I tried to solve the problem that way and got a very different result please check what I did wrong when I attempted this way.
This is my working
The M of A at the new equilibrium is 2 - (2 - [C])/2
The M of B at the new equilibrium is 3 - 3 × (2 - [C])/2
So 4/27 = [C]2/((2 - (2 - [C])/2)×(3 - 3 × (2 - [C])/2)3
From this [C] = 1.24
I don't know why the answer is different, It would be great if you can tell me.
I apologise again for the lack of fractions.
Thanks