The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl].At 550°C, k = 3.2 x 10^-2 sec-1. What is the half-life for this reaction? What was the initialconcentration of ethyl chloride if after one minute, 0.01 M remains?
The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl].At 550°C, k = 3.2 x 10^-2 sec-1. What is the half-life for this reaction? What was the initialconcentration of ethyl chloride if after one minute, 0.01 M remains?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 20QRT
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Question
The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl].
At 550°C, k = 3.2 x 10^-2 sec-1. What is the half-life for this reaction? What was the initial
concentration of ethyl chloride if after one minute, 0.01 M remains?
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