The thiosulfate ion (S2O32-) is oxidized by iodine as follows:2S2O32- (aq) + I2 (aq) → S4O62- (aq) + 2I- (aq)In a certain experiment, 7.05 x 10-3 mol/L of S2O32- is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S2O32-. Calculate the rate of production of iodide ion.

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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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 102CWP: The thiosulfate ion (S2O32) is oxidized by iodine as follows: 2S2O32(aq)+I2(aq)S4O62(aq)+2I(aq) In a...

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The thiosulfate ion (S₂O₃^2-) is oxidized by iodine as follows:

2S₂O₃^2- (aq) + I₂ (aq) → S₄O₆^2- (aq) + 2I^- (aq)

In a certain experiment, 7.05 x 10^-3 mol/L of S₂O₃^2-is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S₂O₃^2-. Calculate the rate of production of iodide ion.

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