In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in chromium(III) ion, Cr3+ Cr3+(aq) + SCN(aq) → Cr(SCN)2+(aq) The rate constant for the reaction is 2.0x10-6/s. How many hours would it take for the concentration of Cr3+ to decrease to 12.5% of its initial concentration? Express your answer to one decimal place.
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in chromium(III) ion, Cr3+ Cr3+(aq) + SCN(aq) → Cr(SCN)2+(aq) The rate constant for the reaction is 2.0x10-6/s. How many hours would it take for the concentration of Cr3+ to decrease to 12.5% of its initial concentration? Express your answer to one decimal place.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.65QP: In the presence of excess thiocyanate ion, SCN, the following reaction is first order in...
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In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in chromium(III) ion, Cr3+
Cr3+(aq) + SCN(aq) → Cr(SCN)2+(aq)
The rate constant for the reaction is 2.0x10-6/s. How many hours would it take for the concentration of Cr3+ to decrease to 12.5% of its initial concentration? Express your answer to one decimal place.
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