(4 points) Your original data, and example calculations, must be recorded in you
ID: 890525 • Letter: #
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(4 points) Your original data, and example calculations, must be recorded in your matches You may use a spreadsheet program to perform your calculations if you wish - attach a copy, instead of filling in the table below. 2 a nice team that the career in musicits we Lumn is that the time since their win in front more Rate Reaction. Temperature (amos time (0) 75 YIOL 3. 15 No2.125 x 104 118s 3. 15 x 2.5x102 125 riots trends in eastern comment on a year reason to 3 7.5x U2 125 rio.125x to 105s soro also has 83s 7.53 XIo 4. 2 poin in what is the order its reactica will cost the same share your calculate 6 as ro325 x - 1 14s HOC 3.41 x 3 1 pelot) Wite the overall take lew thrie Henian SC 5-3 viOS poung Using your data from reactions is calculate an average value for the rate constant your calculation for full credit. 7. (1 points) using the Amrhenius equation, use Excel to prepare a spreadsheet and graph Ink) versus 1/T using your variable temperature data. Ton't forget to convert the temperature to Kelvin. Use the linear trendline finction to determine the values of A and E for this reaction. You should use the spreadsheet math functions to calculate A and E and display them beside your plotAach your spreadsheet, your graph and show your calculations below for full credit.Explanation / Answer
7. To plot lnk vs 1/T your data is not sufficient. Most of the values don't have Temperature input.
Instead, I will calculate Ea from equation,
ln(k2/k1) = Ea/R[1/T1-1/T2]
Consider run 6 and run 7
taking ln of the k values and 1/T1 of temperatures 1/35 oC = 1/308 K and 1/T2 = 1/40 oC = 1/313 K we get,
-10.150/-10.018 = Ea/8.314[0.00325-0.00319]
Ea = 140.392 kJ/mol
2. Calculating rate
rate = -d[S2O8^2-]/dt
lets take run 6 and 7
rate = -(3.15 x 10^-2 - 3.75 x 10^-2)/(16-14) = 0.003 M.s-1
Similarly, rates for other reactants can be calculated.
3. Determining order of reaction,
let, rate = k[I-]^x[S2O8^2-]^y
with x and y be order with respect to I- and S2O8^2-
consider run 1 and run 4
rate1/rate4 = 3.16 x 10^-6/7.53 x 10^-6 = k(7.5 x 10^-2)^x(3.75 x 10^-2)^y/(5 x 10^-2)^x(3.75 x 10^-2)^y
0.420 = 1.5^x
taking log on both sides,
log(0.420) = x log(1.5)
x = 2
So order with respect to I- is 2
4. Now lets consider run 1 and 2, here concentration of I- is same,
rate1/rate2 = 3.16x 10^-6/9.19 x 10^-6 = (3.75 x 10^-2/2.5 x 10^-2)^y
0.344 = 1.5^y
taking log and solving for y,
y = 3
So order with respect to S2O8^2- is 3
5. Overall rate equation becomes,
rate = k[I-]^2[S2O8]^3
with k being the rate constant
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