Please help with this Part A Given the two reactions 1. H2S HS +H K1 -9.34x10-8,

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Please help with this

Part A Given the two reactions 1. H2S HS +H K1 -9.34x10-8, and 2. HS.ts* +H+, K,= 1.17x10-19, what is the equilibrium constant K final for the following reaction? Enter your answer numerically Hints final = Submit My Answers Give Up Part B Given the two reactions 3. PbCl2Pb2+ +2C1, K31.89x10-10, and 4. AgC-Ag+ + Cl-, K4 = 1.25x 10-4. what is the equilibrium constant K final for the following reaction? Express your answer numerically. Hints 0 final = Submit My Answers Give Up

Explanation / Answer

A)
add 1 and 2
H2S <--> 2H+ + S-2
K5 = K1*K2
= 9.34*10^-8*1.17*10^-19
= (1.09*10^-26)

now reverse the obtained reaction
Kfinal = 1/K5
= 1/(1.09*10^-26)
= (9.17*10^25)

B)
multiply the reaction 4 by 2
2AgCl <--> 2Ag+ + 2Cl-
K6 = K4^2
= (1.25*10^-4)^2
= (1.56*10^-8)

now reverse the obtained reaction
2Ag+ + 2Cl- <--> 2AgCl
K7 = 1/K6
= 1/(1.56*10^-8)
= (6.41*10^7)

now add reaction7 and 3
PbCl2 + 2Ag+ <--> 2AgCl + Pb+2
Kfinal = K3*K7
= 1.89*10^-10*(6.41*10^7)
= 1.21*10^-2

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