Given the two reactions. Given the two reactions 3. PbCl(aq) = Pb2+ (aq) + 2CI+ (aq),...
- Part B Given the two reactions 3. PbCl2 (aq) = Pb2+ (aq) + 2C1-(aq), K3 = 1.75x10-10, and 4. AgCl(aq) = Ag+ (aq) + CI+ (aq), K4 = 1.12*10-4 what is the equilibrium constant Kfinal for the following reaction? PbCl2 (aq) + 2Ag+ (aq) = 2AgCl(aq) + Pb2+ (aq) Express your answer numerically.
Given the two reactions PbCl2(s)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.87×10−10, and AgCl(s)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2(s)+2Ag+(aq)⇌2AgCl(s)+Pb2+(aq)
Given the two reactions PbCl2⇌Pb2++2Cl−, K3 = 1.72×10−10, and AgCl⇌Ag++Cl−, K4 = 1.29×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2+2Ag+⇌2AgCl+Pb2+
Part A= Given the two reactions H2S⇌HS−+H+, K1 = 9.42×10−8, and HS−⇌S2−+H+, K2 = 1.32×10−19, what is the equilibrium constant K final for the following reaction? S2−+2H+⇌H2S Part B= Given the two reactions PbCl2⇌Pb2++2Cl−, K3 = 1.89×10−10, and AgCl⇌Ag++Cl−, K4 = 1.23×10−4, what is the equilibrium constant K final for the following reaction? PbCl2+2Ag+⇌2AgCl+Pb2+
1) Given the two reactions: a) H2S<--> HS- + H+, K1=9.13 x 10-8 b) HS-<--> S2- + H+, K2=1.20 x 10-19 what is the equilibrium constant Kfinal for thefollowing reaction? S2- + 2H+<--> H2S 2) Given the two reactions: a)PbCl2 <--> Pb2+ + 2Cl-,K1= 1.80 x 10-10 b) AgCl<--> Ag+ + Cl-, K2= 1.23 x10-4 what is the equilibrium constant Kfinal for thefollowing reaction? PbCl2 + 2Ag+<--> 2AgCl + Pb2+
Learning Goal: 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 K1=[C]c[D]d[A]a[B]b Thus, for a chemical reaction equation with the general form cC+dD⇌eE+fF the equilibrium equation is given by K2=[E]e[F]f[C]c[D]d If the first two equations are added together such that aA+bB⇌eE+fF then the equilibrium equation is given...
1. Write the correct solubility-product expression for the following equilibrium reactions. (a) Pb12 (8) + Pb2+(aq) + 21"(aq) (b) AgCl(s) + Ag (aq) + CI+ (aq) (c) La(IO3)3 (9) + La**(aq) + 3103"(aq)
Consider these two equilibria with their respective equilibrium constants: (1) (2) PbCl2 ()Pb2+ (aq)2CI- (aq) Pbf2 (s) РЬ2+ (aq) + 2 F-(aq) K 1.7x 10-5 K-37x10-8 Which equilibrium will produce more Pb2+ions in solution? B) (2) D) cannot determine with provided information C) both (1) and (2) will produce the same amount
Given the two reactions 1. PbCl2 <=> Pb2+ + 2Cl- K1 = 1.77×10−10, and 2. AgCl <=> Ag+ + Cl- K2 = 1.18×10−4, what is the equilibrium constant for the following reaction?
Part A Given the two reactions 1. H2S(aq) = HS-(aq) + H+(aq), K1 = 9.68x10-8, and 2. HS-(aq) = 32- (aq) +H+(aq), K2 = 1.24x10-19, what is the equilibrium constant Kfinal for the following reaction? 52- (aq) + 2H+(aq) = H2S(aq) Enter your answer numerically.