Na2S203, 1.00 mL of starch solution, and 15.00 mL of 0.110 M (NH)2S,Os to a beak
ID: 703885 • Letter: N
Question
Na2S203, 1.00 mL of starch solution, and 15.00 mL of 0.110 M (NH)2S,Os to a beaker. The volumes are additive. 1. A solution is prepared by adding 15.00 mL of 0.110 M KI, 5.00 mL of 0.0100 M Calculate the concentration of iodide, I, and of peroxydisulfate, S2Os, in the final solution. 0g2- b. Calculate the concentration of thiosulfate, S20,,in the final solution. (0.00500)(0.0100M)= Sfor 10 2. If the reaction described in problem 1 required 103 s for the blue-black color of the starch- iodine complex to appear, calculate the rate of the reaction by using the thiosulfate concentration from lb and Equation (18-4) (0-00139) 03 secors 3. The rate law for the reaction performed in the laboratory exercise was given in Equation (18- 7). Substitute the whole number orders of the reaction with respect to the two reactants that were determined by you in Experiment 18 into the rate law and rearrange the resulting equation to solvefortherate constant k. rate =KCrj'?2082-J k= rate 4. Use the initial concentrations calculated in problem 1, the rate calculated in problem 2 and the equation derived in problem 3 to determine the rate constant, k, of the reaction. 0.15 x10 mo 3.22 x 10 S 5. Data from the Kinetics II experiment will be used to prepare a graph of In(k) vs 1/T. If the reaction described in questions 1-2 of this pre-lab took place at 28°C, what are the x and y values of the data point for this reaction mixture that would be plotted on a graph of In(k) vs 1/T? Remember that temperature in the Arrhenius equation is absolute temperature (Kelvin).Explanation / Answer
Since the first four questions are said to be correct, the value of rate constant is 3.22 x 10-3
The reaction temperature = 28 C = 301.15 K
Here x-axis = 1/T = 1/301.15 == 0.0033 K-1
y-axis = ln K = ln 3.22 x 10-3 = -5.74
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