In: Chemistry
Part A
Given the two reactions
H2S⇌HS−+H+, K1 = 9.02×10−8, and
HS−⇌S2−+H+, K2 = 1.47×10−19,
what is the equilibrium constant Kfinal for the following reaction?
S2−+2H+⇌H2S
Enter your answer numerically.
Hints
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Kfinal= |
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Part B
Given the two reactions
PbCl2⇌Pb2++2Cl−, K3 = 1.81×10−10, and
AgCl⇌Ag++Cl−, K4 = 1.22×10−4,
what is the equilibrium constant Kfinal for the following reaction?
PbCl2+2Ag+⇌2AgCl+Pb2+
Express your answer numerically.
Hints
part A
adding the two given reaction
we get,
H2S < -- > 2H+ + S2-
when we add equlibrium constant of final reaction is product of
equlibrium constant of given
K5 = k1*k2
= 9.02*10^-8*1.47*10^-19
= 1.33*10^-26
so, equlibrium constant of S2−+2H+⇌H2S which is reverse of above
reaction
= 1/K5
= 1/(1.33*10^-26)
= 7.52*10^25
Answer : 7.52*10^25
part B
multiply AgCl⇌Ag++Cl− by 2 we get
2AgCl⇌2Ag++2Cl−
equlibrium constant of these reaction will be square of K4
K6 = (1.22*10^-4)^2
= 1.49*10^-8
now add third reaction and the reaction we got by multiplying by
2
we will get the required one of equlibrium constant K7
k7 = K6*K3
= 1.49*10^-8*1.81×10−10
= 2.70*10^-18
Answer : 2.70*10^-18