Question

G-10 Assume the equilibrium constant K 1 for a reaction A + B 2 C. You prepare a solution that has the following initial concentrations. For each solution, calculate the reaction quotient Q and state if the concentrations of reactants and products will (increase, decrease, or stay the same). a) [A] 1 M, [B] 1M, [C] 2 M. b) [A] 2 M, [B] 1 M,(C] 1 M. Answers: Q 4 >K, [A, B] increase, [C] decreases Q=0.5 < K, [A, B] decrease, [C] increases

Answer 1

Page Data CAIC671x1 ca) [A3 = 14, (B) = 1 m „C)=24 Q = [C]? - (2)=4 So, 0 sk → equilibrium shifte to the left concentration of reactants increases and concentration of products decreases. (6 A1 = 24, [B]-im; [C] = 1M Q=_1472 - 0.5 - CAILB 2X1 w So, Q<K Equilibrium shifts to the right concentration of reactants decreases & of products increases. (as a cro? + 2H+ Cr2 0 2 + H₂O When HNO is added, it gives it lons - no. of it ions in solution increases & Equilibrium shifts to Right (b)|| AgC2H20 Agts + CH3 03 HNOL NOLEH When HNO₃ is added, it from HNO3 combines with acetate Ilons (62130%) to form acetic acid molecules (CH₃ COOH). MNO, is removing C₂H₂0 ions from silver acetate equilibrium » Equilibrium shifts to Right c i Bacau B g2t it Goh Luce - ce + H+ when Hill is added, clions combines with Beet ons to form Ball, He is removing Ba2tions from the barium oxalate equilibrium Equilibrium shifts to right v co o to Co (H2O)]" +40 ² coce 2- + 6H2O . He it tce- I when Hill is added, there are more no of ce ions in the solution Equilibrium shifts to Right