1. The problem statement, all variables and given/known data Initially a mixture contains 0.723 mol each of N2 and O2 in an 7.20 L vessel. Find the composition of the mixture when equilibrium is reached at 3900°C. For the reaction below, the Kc = 0.0123 at 3900°C. N2(g) + O2(g) 2 NO(g) 2. Relevant equations I.C.E Tables (not an equation but relevant) and the quadtratic formula x=-b +or- sq root(b^2 -4ac) / 2a 3. The attempt at a solution I did my I.C.E Table Conc.(M) N2 + O2 --> 2 NO Start 0.6025 0.6025 0 Change -x -x 2x Eq. 0.6025-x 0.6025-x 2x Then I plugged that into my Kc formula Kc=[products]/[reactants] 0.0123=[2x]^2/[0.6025-x][0.6025-x] I then rearranged that to get a quadratic equation to solve for x (this is where I think I made a mistake) -324x^2 -1.205x +0.3630=0 I plugged it into the quadratic formula and got 0.03166 for x, which i plugged into the equations from the EQ. line in my I.C.E table, however when i plugged those values into the Kc formula, i didn't come out with the Kc value I was given (0.0123) Can anyone help?