1. The problem statement, all variables and given/known data The following reaction was allowed to reach the state of equilibrium 2A+B <====> C The initial amounts of reactant present in one litre of solution were 0.5 mole of A and 0.6 mole of B. At equilibrium the amounts were 0.2 mole of A and 0.45 mole of B and 0.15 mole of C. Calculate equilibrium constant 2. Relevant equations Kc= [product]/[reactants] 3. The attempt at a solution Kc= [0.15]/0.2^2×0.45 Kc=0.15/0.018 = 8.3 In my book one of the option of mcq given is 8.3 but the option marked as correct is 11.7 which one is right? If 11.7 is correct then how?