2. The rate constant for the first-order reaction: SO2Cl2(g) = SO2(g) + Cl2(g) is 2.2 x 10–5 s --1. Assume that the initial concentration of SO2Cl2 is 2.00 M. A. What is the half-life? B. How long would it take for the concentration of SO2Cl2 to decrease to 25% of its initial value? C. How long will it take for 12.5% of its initial value to decompose?
2. The rate constant for the first-order reaction: SO2Cl2(g) = SO2(g) + Cl2(g) is 2.2 x 10–5 s --1. Assume that the initial concentration of SO2Cl2 is 2.00 M. A. What is the half-life? B. How long would it take for the concentration of SO2Cl2 to decrease to 25% of its initial value? C. How long will it take for 12.5% of its initial value to decompose?
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 99QRT
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2. The rate constant for the first-order reaction: SO2Cl2(g) = SO2(g) + Cl2(g) is 2.2 x 10–5 s --1. Assume that the initial concentration of SO2Cl2 is 2.00 M.
A. What is the half-life?
B. How long would it take for the concentration of SO2Cl2 to decrease to 25% of its initial value?
C. How long will it take for 12.5% of its initial value to decompose?
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