CHM 123 Due Tuesday 10/17/17 Don\'t forget to show all your work by using integr

Question

CHM 123 Due Tuesday 10/17/17 Don't forget to show all your work by using integrated law and other appropriate formulas/equations or no CREDIT HW -Chapter 13-Chemical Kinetics Name 1. The rate of the reaction, 2 HigCl2 +C20404) 2a(w) +2C020 + 1182Cl2(1), is followed measuring the number of moles of Hg2Cl2 that precipitate per liter per second. The following data are obtained: [HgCl2l 0.10 0.20 IC2041 Initial Rate (mol/L s) 0.10 0.20 0.20 1.3 x 10 5.2 x 10 1.0 x 10 20.10 0.20 a. Write a generic rate law for this reaction rate-k b. Calculate the order of HgCl2 and C204 c. Determine the overall order of reaction d. Write a complete rate law for the reaction with k constant value e. Calculate the necessary [HgCl2) to achieve a rate of 8.0x10 M/s when [C204) 0.35 M

Explanation / Answer

a. rate = k[HgCl2]^x[C2O4^2-]^y

b. order w.r.t HgCl2

   r2/r3 = (a2/a3)^x

(5.2*10^-7/(1*10^-6)) = (0.1/0.2)^x

   x = 0.943 , it is approximately = 1

order w.r.t HgCl2 = x = 1

order w.r.t C2O4^2-

r1/r2 = (a1/a2)^y

(1.3*10^-7/(5.2*10^-7)) = (0.1/0.2)^y

   order w.r.t C2O4^2- = y= 2

c. overall order of reaction = 1+2 = 3

d. rate = k[HgCl2]^1[C2O4^2-]^2

   k = rate / [HgCl2]^1[C2O4^2-]^2

     = (1.3*10^-7)/(0.1*0.1^2)

     = 1.3*10^-4 M-2.S-1

e. rate = k[HgCl2]^1[C2O4^2-]^2

8*10^-4 = (1.3*10^-4)*X*0.35^2

X = [HgCl2] = 50.23 M

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