aA + 6B cC + dD the equilibrium equation is given by K1 = [C]c[D]d / [A]a [B]b T

Question

aA + 6B 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 or K3 = K1 middot 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. Given the two reactions H2S HS- + H+ , K1 = 9.22 times 10-8, and HS- + S2- + H+ , K2 = 1.43 times 10-19, what is the equilibrium constant K final for the following reaction? S2- + 2H+ H2S Enter your answer numerically. Given the two reactions PbCl2 Pb2+ + 2C1-, K3 = 1.88 times l0-10, and AgCl Ag+ + Cl- , K4 = 1.18 times 10-4, what is the equilibrium constant K final for the following reaction? Express your answer numerically.

Explanation / Answer

Part A To get the final reaction you have to reverse both initialreactions. When reversing them, K is inversed! (1 / K1) * (1 / K2) = 7.584606283 *1023 Part B To get the final reaction, the second reaction has to bereversed and doubled. When doubling you square, and reversing youinverse! (K1) * (1 / K2)2 = 0.0135018673

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