Question

In CCl4 solvent, the reaction I + I → I2 is second order in the concentration of iodine atoms. The rate constant k has been measured as 6.53×109 M-1 s-1. Suppose the initial concentration of I atoms is 8.96×10-5 M. Calculate their concentration after 2.23×10-6 s. [I] after 2.23×10-6 s

Name: in ccl4 solvent the reaction i i i2 is second order in the concentration of iodine atoms the rate constant k has been measured as 653109 m 1 s 1 suppose the initial concentration of i atoms 54928
Uploaded: 2022-02-06T12:53:05-08:00
Duration: 2 min 56 s
Channel: Reema C
Description: in ccl4 solvent the reaction i i i2 is second order in the concentration of iodine atoms the rate constant k has been measured as 653109 m 1 s 1 suppose the initial concentration of i atoms 54928

          In CCl4 solvent, the reaction
I + I → I2
is second order in the concentration of iodine atoms. The rate constant k has been measured as 6.53×109 M-1 s-1.
Suppose the initial concentration of I atoms is 8.96×10-5 M. Calculate their concentration after 2.23×10-6 s.
[I] after 2.23×10-6 s

Added by Jeremy M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Reema C

02/06/2022

Step 1

To calculate the concentration of iodine atoms \([I]\) after a given time for a second-order reaction, we can use the integrated rate law for a second-order reaction: \[ \frac{1}{[I]} - \frac{1}{[I_0]} = kt \] where: - \([I]\) is the concentration of iodine atoms Show more…

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In CCl4 solvent, the reaction I + I → I2 is second order in the concentration of iodine atoms. The rate constant k has been measured as 6.53×109 M-1 s-1. Suppose the initial concentration of I atoms is 8.96×10-5 M. Calculate their concentration after 2.23×10-6 s. [I] after 2.23×10-6 s