Given the two reactions 3. PbCl2 (aq) = Pb2+ (aq) + 2Cl(aq), K3 = 1.76x10-10, and 4. AgCl(aq) = Ag+ (aq) + Cl- (aq), K4 = 1.12x10-4, what is the equilibrium constant Kfinal for the following reaction? PbCl2 (aq) + 2Ag+ (aq) = 2AgCl(aq) + Pb2+ (aq) Express your answer numerically. View Available Hint(s) RE VAO Kfinal = 5.07 1013 Submit Previous Answers Request Answer * Incorrect; Try Again; 3 attempts remaining To understand how to calculate the equilibrium constants for chemical equations that can be produced by the addition of other chemical equations with known equilibrium constants. For a chemical reaction equation with the general form aA + bB =cC+ dD the equilibrium equation is given by [C]*[D]" [A]"B Thus, for a chemical reaction equation with the general form cC + dD=eE+fF the equilibrium equation is given by [E]"[F]' [C"D" * If the first two equations are added together such that K - K2= QA+bB=eE+fF then the equilibrium equation is given by [E]'F' C'DE'F JA"B A" BC"D" K3 or K3 = KK Thus, when a chemical equation is the sum of two chemical equations for which equilibrium constants are already known, the equilibrium constant for the reaction is the product of the equilibrium constants for the individual reactions. Keep in mind that equilibrium equations do not include expressions for any pure solids or liquids that may be involved in the reaction