Problem: Iodine atoms will combine to form I2 in liquid hexane solvent with a rate constant of 1.5 x 1010 L/mol•s. The reaction is second order in I. Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial [ I ] concentration of 2.00 x 10−2 M. How long will it take for 92% of the newly created iodine atoms to recombine to form I2?

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We’re being asked to determine the time needed for 92% of I atoms to recombine to I2 given the following second-order reaction:

2 I  I2


The integrated rate law for a second-order reaction is as follows:


1[A]t=kt+1[A]0


where: 

[A]t = concentration at time t

k = rate constant

t = time (unknown)

[A]0 = initial concentration



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Problem Details

Iodine atoms will combine to form I2 in liquid hexane solvent with a rate constant of 1.5 x 1010 L/mol•s. The reaction is second order in I. Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial [ ] concentration of 2.00 x 10−2 M. How long will it take for 92% of the newly created iodine atoms to recombine to form I2?

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