Part A Given the two reactions H2SHS+H+, K1 = 9.14×10^8, and HSS2+H+, K2 = 1.03×

Question

Part A

Given the two reactions H2SHS+H+, K1 = 9.14×10^8, and HSS2+H+, K2 = 1.03×10^19, what is the equilibrium constant Kfinal for the following reaction? S^2+2H+H2S

Enter your answer numerically. Kfinal =

Part Part B

Given the two reactions PbCl2Pb^2+ +2Cl^, K3 = 1.73×10^10,

and AgClAg^+ +Cl^, K4 = 1.19×10^4, what is the equilibrium constant Kfinal for the following reaction? PbCl2+2Ag+2AgCl+Pb^2+

Express your answer numerically.

Kfinal =

Item 14

The equilibrium constant for the reaction shown here is Kc=1.1×103. A reaction mixture at equilibrium contains [A]=2.6×103 M .
A(g)B(g)

Part A

What is the concentration of B in the mixture?

Express your answer using two significant figures.

Item 14

The equilibrium constant for the reaction shown here is Kc=1.1×103. A reaction mixture at equilibrium contains [A]=2.6×103 M .
A(g)B(g)

Part A

What is the concentration of B in the mixture?

Express your answer using two significant figures.

Explanation / Answer

1)A) K1=9.14*10^-8

K2=1.03*10^-19

so,

Kreaction = 1/(k1*K2)

=1.06*10^43

B) Kfinal= K3/(K4^2)

=1.73*10^-10/(1.19*10^-4)^2

=0.0122

14)A) Keq=[Beq]/[Aeq]

or x/2.6*10^-3=1.1*10^3

or x=2.86 M=[Beq]

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