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Experimental Data All the data used in the graphs and calculations to follow is accumulated in the following chart. Calculate the concentrations of persulfate, S208², and iodide, I, in the final reaction mixture after mixing. (Use M₁ V₁ = M₂V₂. The drops of starch can be ignored in the final volume. Calculations 8 0 -1 -2 -4 Reaction 1 2 1 2 3 4 -5- 3 4 Equation of line log rate vs. log after mixing 5 6 -1.6 7 8 9 10 11 [S₂0² ]After mixing 16 09 .00 08 104 .08 -08 .08 -08 -08 Part A; Determination of the orders of reaction, m and n. Using reactions 1, 2, 3 and 4 determine m, the order of the reaction with respect to persulfate, $208². Complete the table below, then plot a graph of log(rate) vs log[S2082²], and draw a linear trendline through the points. The slope of this line is m Reaction [S₂08² ]After mixing log rate -1.02x-3.23 [After mixing 08 -1.2 -08 -0.8 log after mixing .00 08 .DX log[S₂08² ]After mixing -.796 -1.096 -1.348 -1.699 OY -1.0 Temp, °C 25° Time, s 30 10 58.89 5° 15° - ACS₂03 st 111.79 -0.8 Time, s 13.18 30.10 58.89 111 79 15.66 112.35 183 72.2 2.10 1-25×10 Rate, Ms-1 log[Rate] 1-4.02 4.15×10 2.12× 10 -4.67 1.12 x 10-4.95 m= 1-02
1-25 x 163 3 of 10 Use reactions 2, 5, 6 and 7 to determine n, the order of the reaction with respect to iodide, I. Complete the table below, then plot a graph of log(rate) vs log, and draw a linear trendline through the points. The slope of this line is n Reaction 2 5 6 7 Equation of line After mixing 16 -04 rate of ralez -1 log rate vs. log after mixing -2 Z 3 -1.6 log[1]After mixing -1.0969 rate 1 = 9.98×10²³ [16] [108] ¹5 457 -0.7959 -1.3979 -1.6989 Reaction [S₂08²-] After mixing 1 2 6 108 log rato 0.957 K+-3.33 Calculation of k for reaction 1 rate= K[S₂] [I -1.4 4-15x10-5 (ory (on) 157 2.08x10-5 -08) Lod 12 log atar mixing 157 .04) 15 Calculation of rate constants Using the values of m and n, calculate the values of the rate constant, k, for reactions 1, 2 and 6. Show the work for the calculation of the rate constant for reaction 1 only. Complete the chart below with the rate constants for the other reactions Time, s 30 04 40 15.66 60.03. 112.35 -1.0 After mixing Rate, Ms¹ 4.17 x 10-1 7.98, 10 2.08, 10 -0.8 k 5.48,105 log[Rate] -4.38 4.87 10 5 1.26 x 10-5 4.68 -4.95 n- .957
Part B. Effect of Temperature In reactions 2, 8, 9 and 10, the rates were measured at different temperatures, using the same concentrations of reactants. This will allow the activation energy of the reaction to be determined. Note the relationship between increased temperature and the rate of reaction. The Arhenius equation is: Reaction 2 8 9 10 Equation of line: Complete the table below, then plot a graph of Ink vs 1/T (in kelvin), using data from reactions 2, 8, 9 and 10. Fit a linear trendline to the graph and determine the slope of the line. Determine the activation energy from the slope of the line, (Slope = -E/R), and the value of A, from the intercept. E₁ = k Calculation of activation energy Ink - Ea 1 R T + InA Ink A Temp, K 1/T, K-1