± Adding Equilibrium Reactions
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+bBâcC+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+dDâeE+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+bBâeE+fF
then the equilibrium equation is given by K3=[E]e[F]f[A]a[B]b=[C]c[D]d[A]a[B]bâ [E]e[F]f[C]c[D]d
or K3=K1â K2
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.
Part A
Given the two reactions H2SâHSâ+H+, K1 = 9.86Ã10â8, and
HSââS2â+H+, K2 = 1.25Ã10â19,
what is the equilibrium constant Kfinal for the following reaction? S2â+2H+âH2S
Enter your answer numerically.
Kfinal = 7.14â¢1025
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Part B
Given the two reactions PbCl2âPb2++2Clâ, K3 = 1.76Ã10â10, and
AgClâAg++Clâ, K4 = 1.13Ã10â4,
what is the equilibrium constant Kfinal for the following reaction? PbCl2+2Ag+â2AgCl+Pb2+
Express your answer numerically.
Kfinal =
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± Adding Equilibrium Reactions 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+bBâcC+dD the equilibrium equation is given byK1=[C]c[D]d[A]a[B]b Thus, for a chemical reaction equation with the general form cC+dDâeE+fF the equilibrium equation is given byK2=[E]e[F]f[C]c[D]d If the first two equations are added together such thataA+bBâeE+fF then the equilibrium equation is given byK3=[E]e[F]f[A]a[B]b=[C]c[D]d[A]a[B]bâ [E]e[F]f[C]c[D]d orK3=K1â K2 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. | Part A Given the two reactionsH2SâHSâ+H+, K1 = 9.86Ã10â8, and HSââS2â+H+, K2 = 1.25Ã10â19, what is the equilibrium constant Kfinal for the following reaction?S2â+2H+âH2S Enter your answer numerically.
SubmitHintsMy AnswersGive UpReview Part Incorrect; Try Again; 4 attempts remaining Part B Given the two reactionsPbCl2âPb2++2Clâ, K3 = 1.76Ã10â10, and AgClâAg++Clâ, K4 = 1.13Ã10â4, what is the equilibrium constant Kfinal for the following reaction?PbCl2+2Ag+â2AgCl+Pb2+ Express your answer numerically.
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