I need help with my Kinetics Lab. I need to determine the Rate of the Reaction (
ID: 837701 • Letter: I
Question
I need help with my Kinetics Lab. I need to determine the Rate of the Reaction (M/sec) and k (need to determine units). Below is my lab data. I am asking that you show me/explain how to determine the Rate of the Reaction and then k using the data below. I need to figure this out! Thank you!
Run #
[KI]
(M)
[Na2S2O3]
(M)
[(NH4)2S2O8]
(M)
Time
(seconds)
Rate of Reaction
(M/sec)
Temp
(K)
K
1
0.075
0.00044
0.01875
84
294.15
2
0.050
0.00044
0.01875
111
294.15
3
0.025
0.00044
0.01875
266
294.15
4
0.075
0.00044
0.0125
97
294.15
5
0.075
0.00044
0.00625
223
294.15
6
0.075
0.00044
0.01875
36
306.15
7
0.075
0.00044
0.01875
106
282.15
8
0.075
0.00022
0.01875
40
294.15
Run #
[KI]
(M)
[Na2S2O3]
(M)
[(NH4)2S2O8]
(M)
Time
(seconds)
Rate of Reaction
(M/sec)
Temp
(K)
K
1
0.075
0.00044
0.01875
84
294.15
2
0.050
0.00044
0.01875
111
294.15
3
0.025
0.00044
0.01875
266
294.15
4
0.075
0.00044
0.0125
97
294.15
5
0.075
0.00044
0.00625
223
294.15
6
0.075
0.00044
0.01875
36
306.15
7
0.075
0.00044
0.01875
106
282.15
8
0.075
0.00022
0.01875
40
294.15
Explanation / Answer
The slowest step determines the measured reaction rate, and is called the rate-determining step and in this reaction
2 I? + S2O8?2 ? I2 + 2 SO4?2 is the rate determining step
Rate = ??[I?] / 2?t since two I ions react we have a 2 in the denominator
after we get the rate...
Rate = k[I?]x[S2O82?]y
The exponents x and y must be determined by experiment values
For example, if we double the initial [I-] and
1.) the rate does not change, then x must be equal to zero, zero order...
2.)nIf Rate doubles then x=1 first order ..
3.) if rates becomes 4 times then x =2
similarly we find y..
we now have R and x ,y.. we can find k from the rate equation
this is how it has to be done..
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