1. The problem statement, all variables and given/known data Rxn: 2SO2 (g) + O2 (g) [itex]\Leftrightarrow[/itex] 2SO3 (g) If the initial concentration of SO3 is .500 M (moles/liter) @1500K, what are the final concentrations of [SO2], [O2] and [SO3]. Kc = .15 Stop when you get to the cubic equation 2. Relevant equations RICE table Kc= [SO3]2/ [O2][SO2]2 This is equilibrium quotient for forward reaction. I will flip it to get reverse reaction Kc equation 3. The attempt at a solution This is the Kc given for the forward reaction. If I flip the reaction around I invert the Kc and it becomes = 6.6667 (for the reverse reaction) I then used a "rice" table with the initial concentration of SO3 and "x" variable for the SO2 and O2[ Plugging these values in I get the kc equation: 6.6667= [2x]2[x]/[.500-2x] I'm not getting the correct cubic equation when expanding this quotient. I'm sure of my math, so I was wondering if i'm setting up the quotient wrong? - Thanks!