### Chemical Reaction Analysis#### Oxidation of Thiosulfate Ion by IodineThe thiosulfate ion \((\text{S}_2\text{O}_3^{2-})\) is oxidized by iodine as follows:\[ 2\text{S}_2\text{O}_3^{2-} (\text{aq}) + \text{I}_2 (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} (\text{aq}) + 2\text{I}^- (\text{aq}) \]#### Experimental DataIn a certain experiment, \( 8.13 \times 10^{-3} \, \text{mol/L} \) of \( \text{S}_2\text{O}_3^{2-} \) is consumed in the first 11.0 seconds of the reaction.#### CalculationCalculate the rate of consumption of \( \text{S}_2\text{O}_3^{2-} \).\[ \boxed{\_\_\_\_\_\_\_} \, \text{mol L}^{-1} \text{s}^{-1} \]

The rate of consumption if thiosulphate ion can be calculated by dividing consumed amount by change…

The thiosulfate ion (S,O3-) is oxidized by iodine as follows: 25,032(aq) + I5(aq) S406(aq) + 21(aq) In a certain experiment, 8. 13 10 mol/L of S,O3 is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S,O3. mol/L/s

The thiosulfate ion (S,O3-) is oxidized by iodine as follows: 25,032(aq) + I5(aq) S406(aq) + 21(aq) In a certain experiment, 8. 13 10 mol/L of S,O3 is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S,O3. mol/L/s

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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