Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to the following unbalanced equation: In+(aq) = In(s) + In3+(aq) This disproportionation follows first-order kinetics with a half-life of 667 s. What is the concentration of In+(aq) after 1.35 h if the initial solution of In+(aq) was prepared by dissolving 2.38g InCl(s) in dilute HCl to make 5.0x10^2 mL of solution? What mass of In(s) is formed after 1.35 h?

Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to the following unbalanced equation: In+(aq) = In(s) + In3+(aq) This disproportionation follows first-order kinetics with a half-life of 667 s. What is the concentration of In+(aq) after 1.35 h if the initial solution of In+(aq) was prepared by dissolving 2.38g InCl(s) in dilute HCl to make 5.0x10^2 mL of solution? What mass of In(s) is formed after 1.35 h?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 89IL: The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) +...

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