Chemistry

Given the two reactions

1.PbCl2 <--->Pb^2+ + 2 Cl^-,
K1= 1.82×10^−10

2. AgCl <----> Ag^+ + Cl^-,
K2 = 1.15×10−4

what is the equilibrium constant Kfinal for the following reaction?

PbCl2+ 2 Ag^+ <---> 2AgCl+ Pb^2+

This is what i have soo far:

PbCl2<--->Pb2+ + 2Cl- K1= 1.82×10^−10
AgCl <---> Ag+ + Cl- K2= 1/1.15×10^−4

(AgCl)^2(Pb)/(PbCl2)(Ag)2=
(Pb2+)(Cl)^2/(PbCl2)* (Ag)(Cl-)/(AgCl)

I dunt know what to do next because, i did :

= 1.82×10^−10 * 1/1.15×10^−4
and the answer is wrong,

It says When the stoichiometry of a reaction changes, the new equilibrium constant is raised to the same power. Thus, if a reaction is multiplied by 2, the equilibrium constant K is squared.

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  1. Right. First, however, check your numbers for the k values. I think they are reversed because Ksp for AgCl is about 10^-10 and Ksp for PbCl2 is about 10^-4. But if the Ks were put in the problem on purpose, then
    K1 = 1.82 x 10^-10
    and K2 for the reverse direction is 1/1.15 x 10^-4 and you square that [that is (1/K2)^2].
    Since you added the equations to get the final equation, now you multiply the new Ks. So K for the reaction requested is K1/K2^2. Check me out on that.

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  2. The Values are correct i doubled checked:

    But when do

    1.82 x 10^-10/ (1/1.15×10^−4)^2
    = 2.47*10^-18

    But it says this answer is wrong

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  3. No.
    K1 = 1.82 x 10^-10
    K2 = (1/1.15 x 10^-4)^2
    Then Keq for the reaction is
    K1*(1/K2)^2 =
    1.82 x 10^-10*(1/1.15 x 10^-4)^2 =
    1.82 x 10^-10*(7.56 x 10^7) =
    0.01376. Check it for math. Check it for significant figures.

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  4. I would round it ti 0.014 = Keq.

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  5. Here is the error
    So K for the reaction requested is K1/K2^2. Check me out on that.
    It's K1*(1/K2)^2
    1.82 x 10^-10*(1/1.15 x 10^-4)^2 = 0.014

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  6. That's right thank you

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