The following reaction initially contains [A]o = 0.2150 M and o = [C]o = 0.4150 M. If the equilibrium constant for the reaction is Keq = 2.03, what are the concentrations of reactants and products when the reaction has achieved equilibrium? What is the value of deltaG for the reaction at 25oC?
2 A <-> B + C
I am stuck as on how to proceed with the math. I'm not sure if I am doing it correctly or not. Could someone please take a look?
The Attempt at a Solution
Initial: 2A B C
0.2150M 0.4150M 0.4150M
Change: +x -x -x
Since Q>Kc, as Qc = [C]/[A]^2
Equil. 0.2150+x 0.4150-x 0.4150-x
I'm stuck on the whole rearranging and solving for x bit. I know I'm supposed to use quadratic formula.