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viridianbeetle50Lv1

6 Nov 2019

In the reaction between H2O2 and I^-, 15 ml of 0.30 M KI, 68 ml of 0.10 M H2O2and 19 ml 0.020 M Na2S2O3 were mixed in a flask containing starch and buffer and the total volume was made up to 500 ml with distilled water. The solution turned blue 9 indicating the presence of I2) in 1.8 minutes. Calculate the initial rate of disappearance of H2O2 in units of M min^-1 to two significant figures.

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Related questions

1. For the reaction A + B --> C, the rate law is rate = k[A]. If the initial concentration of A = 2.4 mol/L, the initial [B] = 1.4 mol/L, and the rate = 0.57 moles of product per litre per minute (M/min). Calculate the rate constant k to 2 decimal places.

2. In the reaction between H2O2 and I-, 15 mL of 0.30M KI, 71. mL of 0.10M H2O2 and 19 mL of 0.020M Na2S2O3 were mixed in a flask containing starch and buffer and the total volume was made up to 500mL with distilled water. The solution turned blue (indicating the presence of I2) in 1.9 minutes. Calculate the initial rate of disappearance of H2O2 in units of M min-1 to two significant figures. Hint: there are two reactions occuring here as represented by the equations 1 and 4 in the introduction of the lab manual procedure for this experiment.

Add 25 mL of 0.010 M of Na2S2O3, another 25 mL of buffer solution, and 25 mL of 0.1% starch stock solution. Then in the same flask, add 25 mL of 0.060 M of KI, 30 mL of distilled water, and 20 mL of 0.040 M of H2O2.

Please calculate the initial molarity of Thiosulfate ion in this reaction mixture.

353 Table 1: Grid indicating the solutions to add for each initial rate experiment: | Initial rate experiment1 Initial rate experiment 2 Initial rate experiment 3 10.0 mt Kfterg)_v 10.0 mL KI(aq 5.0 mL KI(aq) v Add first 5.0 mL Na2S2O3(aq) 5.0 mL Na2S;Ostag 5.0 mL Na2S2O3(aq) 10 mL starch(aq) 5.0 mL NaCl(aq) v 1.0 mL starch(aq) 1.0 mL starch(aq) v Add last, 10.0 mL K2S2O3(aq) start timer 5.0 mL K2S2O3(aq) 10.0 mL KS203(aq) Part A: Determination of rate law Y Collect the following solutions in separate small, clean, and dry beakers (label them!): 15-20 mL of 0.10 M Na2SO4 130 mL of 0.10 M KI 15-20 mL of 0.10 M NaCI 130 mL of 0.10 MK28208 15-20 mL of starch solution SV Obtain three large (25 x 200 mm) test tubes, and make sure that they are clean and as dry as possible. You will also need a digital thermometer and a timer. . You will perform three initial rates experiments. Table 1 provides the final contents for each of three initial rates experiments. You will set up and run three trials for each initial rates experiment in the three test tubes. For each initial rates experiment: . Add the amount of KI solution indicated in Table 1 using a digital pipette to the three test tubes. Rinse the pipette tip with distilled water. b. Where required, add the indicated amounts of NaCl and Na2SO4 solutions using the digital pipette to the three test tubes. Rinse the pipette tip with distilled water between solutions. c. Add 1.0 mL of starch solution using the digital pipette to each one of the three test tubes. Rinse the pipette tip with distilled water. d. Add 5.0 mL Na2S2O3 solution using the pump dispenser to each one of the three test tubes. e. Do the following one test tube at a time for all three test tubes: Start the timer as you deliver the indicated amount of K2520s solution using the digital pipette. Stir the solution at a constant rate using a digital thermometer - consistency in your rate of stirring for all initial rates experiments is important! Stop the timer at the first sign that the solution has turned blue-black, and record time and the temperature at this point. - OT Ask your TA to check your data for Part A before starting Part 3 + = 1956Â°C XÄ± NaaS303, Stoch. Clar 19.4Â°C SOSec

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