Data were collected to determine the rate law for the reaction iodide with hydro
ID: 484389 • Letter: D
Question
Data were collected to determine the rate law for the reaction iodide with hydrogen peroxide. The following data were collected for Kinetic Trial 1. See the Experimental Procedure, Part B, and the Report Sheet for completing the following table. Record the calculated values with the correct numbers of significant figures. Determination of Reaction Times Molar concentration of Na_2S_2O_3(L) Ambient temperature (degree C) Molar concentration of KI (mol/L) Molar concentration of H_2O_2 (mol/L) Total volume of kinetic trial (mL) Time for color change. Delta t (sec) Calculations for Determining the Rate Law Moles of S_2O_3^2- consumed (mol) Show calculation. Delta (mol I_3^-) produced Equation 24, 11 Show calculation. Delta (mol I_3^-)/Delta t (mol/sec) Show calculation. log Delta(mol I_3^-)/Delta t Show calculation. Volume KI(mL) [I^-]_o (mol/L)** Show calculation. Not 0.3 M. See footnote 6. log[I^-]_o Volume of H_2O_2 (mL) [H_2O_2] (mol/L)** Show calculation. Not 0.1 M. See footnote 7. log [H_2O_2] **See the second page of the Report Sheet to determine the further use of this data.Explanation / Answer
From the given data values,
1. moles of S2O3^2- = 0.02 M x 0.001 L = 2 x 10^-5 mols
2. moles[I3-] produced = 2 x 10^-5/2 = 1 x 10^-5 mols
3. d[I3-]/dt = 1 x10^-5/25 = 4 x 10^-7 M/s
4. log(d[I3-]/dt) = -6.4
5. volume KI = 2 ml [this volume is assumed, you need to feed exact starting volume of KI taken]
6. [I-]o = 0.3 M x 0.002 L/0.01 = 0.06 mols/L
7. log[I-]o = -1.22
8. volume H2O2 = 1 ml [let the volume be 1 ml, you need to feed the exact starting volume of H2O2 taken]
9. [H2O2] = 0.1 M x 0.001 L/0.01 = 0.001 mols/L
10. log[H2O2] = -3
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