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 for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.45PAE: The initial concentration of the reactant in a tirst-order reaction A —» products is 0.64 rnol/L and...
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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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