To understand how to calculate the equilibrium constants for chemical equations

Question

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 by K3 = [E]e[F]f/[A]a[B]b = [C]c[D]d/[A]a[B]b middot [E]e[F]f/[C]c[D]d Given the two reactions PbCl2 Pb2+ + 2Cl-, K3 = 1.82 times 10-10, and AgCl Ag+ + Cl-, K4 = 1.13 times 10-4 what is the equilibrium constant Kfinal for the following reaction? PbCl2 + 2Ag+ 2AgCl + Pb2+

Explanation / Answer

equation( 3)-2*equation(4)=given equation so Kfinal=K3 * K4 ^(-2) =K3/(K4)^2

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