Iodine atoms combine to form molecular iodine in the gas phaseThis reaction follows second-order kinetics and has the high rate constant 7.0 x 10°/M s at 23°C.If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min.(a)(b) Calculate the half-life of the reaction if the initial concentration of I is 0.60 M and if it is 0.42 M.BStrategy(a)I(g) + I(g) → 12 (8)(b)11+1—hPage 589The relationship between the concentrations of a reactant at different times is given by the integrated rate law. Becausethis is a second-order reaction, we use Equation (13.7).We are asked to calculate the half-life. The half-life for a second-order reaction is given by Equation (13.8).

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Todine atoms combine to form molecular iodine in the gas phase I(g) + I(g) → 1₂ (g) This reaction follows second-order kinetics and has the high rate constant 7.0 x 10°/M s at 23°C. (a) If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. (b) Calculate the half-life of the reaction if the initial concentration of I is 0.60 M and if it is 0.42 M.

Todine atoms combine to form molecular iodine in the gas phase I(g) + I(g) → 1₂ (g) This reaction follows second-order kinetics and has the high rate constant 7.0 x 10°/M s at 23°C. (a) If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. (b) Calculate the half-life of the reaction if the initial concentration of I is 0.60 M and if it is 0.42 M.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Iodine atoms combine to form molecular iodine in the gas phase
This reaction follows second-order kinetics and has the high rate constant 7.0 x 10°/M s at 23°C.
If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min.
(a)
(b) Calculate the half-life of the reaction if the initial concentration of I is 0.60 M and if it is 0.42 M.
B
Strategy
(a)
I(g) + I(g) → 12 (8)
(b)
1
1+1—h
Page 589
The relationship between the concentrations of a reactant at different times is given by the integrated rate law. Because
this is a second-order reaction, we use Equation (13.7).
We are asked to calculate the half-life. The half-life for a second-order reaction is given by Equation (13.8).

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