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Chemistry

I already answered the first three questions and put theanswer down I just don't know how to answer the last question whichasks to calculate K in the rate law?
A clock reaction is run at 20 ÂºC with several different mixturesof iodide, sodium bromate and acid, to form iodine. Thiosulfate isused to react with the iodine formed initially. Starch indicator isadded to form a blue color when all the thiosulfate has been usedup and the iodine concentration begins to rise. The following setsof mixtures are used.

Initial concentrations in reaction mixtures
Run number [I^-]Â Â Â Â Â [BrO₃^-]Â Â Â Â [H⁺]
1 0.002Â Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â 0.02
2 0.002 Â Â Â Â Â 0.016Â Â Â Â Â Â Â Â Â Â 0.02
3 0.004 Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â 0.02
4 0.002 Â Â Â Â Â Â 0.008Â Â Â Â Â Â Â Â Â Â Â 0.04 Â Â
[S₂O₃^2- ] is equal to 0.0001M ineach reaction mixture.
The rate law is :
Â Â
Rate = k [ I^-]^aÂ Â [BrO₃^-]^bÂ Â [H⁺]^c

Reaction time in run number 1 30
Reaction time in run number 2 30
Reaction time in run number 3 15
Reaction time in run number 4 30

Calculate the following
a in the rate law
a=1
A clock reaction is run at 20 ÂºC with several different mixturesof iodide, sodium bromate and acid, to form iodine. Thiosulfate isused to react with the iodine formed initially. Starch indicator isadded to form a blue color when all the thiosulfate has been usedup and the iodine concentration begins to rise. The following setsof mixtures are used.

Initial concentrations in reaction mixtures
Run number [I^-]Â Â Â Â Â [BrO₃^-]Â Â Â Â [H⁺]
1 0.002Â Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â 0.02
2 0.002 Â Â Â Â Â 0.016Â Â Â Â Â Â Â Â Â Â 0.02
3 0.004 Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â 0.02
4 0.002 Â Â Â Â Â Â 0.008Â Â Â Â Â Â Â Â Â Â Â 0.04 Â Â
[S₂O₃^2- ] is equal to 0.0001M ineach reaction mixture.
The rate law is :
Â Â
Rate = k [ I^-]^aÂ Â [BrO₃^-]^bÂ Â [H⁺]^c

Reaction time in run number 1 30
Reaction time in run number 2 30
Reaction time in run number 3 15
Reaction time in run number 4 30

Calculate the following
b in the rate law
b=0
A clock reaction is run at 20 ÂºC with several different mixturesof iodide, sodium bromate and acid, to form iodine. Thiosulfate isused to react with the iodine formed initially. Starch indicator isadded to form a blue color when all the thiosulfate has been usedup and the iodine concentration begins to rise. The following setsof mixtures are used.

Initial concentrations in reaction mixtures
Run number [I^-]Â Â Â Â Â [BrO₃^-]Â Â Â Â [H⁺]
1 0.002Â Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â 0.02
2 0.002 Â Â Â Â Â 0.016Â Â Â Â Â Â Â Â Â Â 0.02
3 0.004 Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â 0.02
4 0.002 Â Â Â Â Â Â 0.008Â Â Â Â Â Â Â Â Â Â Â 0.04 Â Â
[S₂O₃^2- ] is equal to 0.0001M ineach reaction mixture.
The rate law is :
Â Â
Rate = k [ I^-]^aÂ Â [BrO₃^-]^bÂ Â [H⁺]^c

Reaction time in run number 1 30
Reaction time in run number 2 30
Reaction time in run number 3 15
Reaction time in run number 4 30

Calculate the following
c in the rate law
C=0
If the rate law for the clock reaction is:
Â Â Â
Rate = k [ I^-] [ BrO₃^-][H⁺]
A clock reaction is run with the following initialconcentrations:
[I^-] Â Â Â Â Â Â Â Â Â Â Â Â [BrO₃^-] Â Â Â Â Â Â Â Â Â Â [H⁺]Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â [S₂O₃^2-]
0.002 Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.008Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.02Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.0001Â Â
The reaction time is 28 seconds
Calculate k in the rate law:?

Answer & Explanation Solved by verified expert

3.6 Ratings (266 Votes)

Rate = k [ I-]aÂ Â [ BrO3-]bÂ Â [H+]c

calculation of \"a\"

using the values that you have calculated for b and c and dviding rate expression obatined in trial 2 by that in 3.

we get (1/2)a = 1/2; which shows a = 1.

putting these values of a= 1, b=0, and c= 0 in rate law

rate = k[I-]

reaction is first order w.r.t [I-]

Now,

using initial concentrations:

[I-] Â Â Â Â Â Â Â Â Â Â Â Â [BrO3-] Â Â Â Â Â Â Â Â Â Â [H+]Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â [S2O32-]
0.002 Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.008 Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.02 Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.0001Â Â

The reaction time is 28 seconds to alculate k.

(0.0001/28) Ms-1 = k (0.002) M

k = 1.78 x 10-3 s-1

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