Question

Iodine atoms combine to form molecular iodine in the gas phase. The reaction is second order and has a rate constant of 7.0 × 10^9 M^–1 · s^–1 at 23°C. If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. Calculate the half-life of the reaction when the initial concentration of I is 0.60 M and when the initial concentration of I is 0.42 M.

Name: iodine atoms combine to form molecular iodine in the gas phase the reaction is second order and has a rate constant of 70 109m1 s1 at 23c if the initial concentration of i is 0086 m calculat 80154
Uploaded: 2022-02-06T12:53:05-08:00
Duration: 2 min 56 s
Channel: Reema C
Description: iodine atoms combine to form molecular iodine in the gas phase the reaction is second order and has a rate constant of 70 109m1 s1 at 23c if the initial concentration of i is 0086 m calculat 80154

          Iodine atoms combine to form molecular iodine in the gas phase. The reaction is second order and has a rate constant of 7.0 × 10^9 M^–1 · s^–1 at 23°C. If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. Calculate the half-life of the reaction when the initial concentration of I is 0.60 M and when the initial concentration of I is 0.42 M.

Added by Sandra H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Reema C

02/06/2022

Step 1

0 min using the given initial concentration of I (0.086 M) and rate constant (7.0 × 10^9 M^–1 · s^–1). Given: Initial concentration of I (I₀) = 0.086 M Rate constant (k) = 7.0 × 10^9 M^–1 · s^–1 Time (t) = 2.0 min = 2.0 × 60 s = 120 s Using the second-order rate Show more…

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Iodine atoms combine to form molecular iodine in the gas phase. The reaction is second order and has a rate constant of 7.0 × 10^9 M^–1 · s^–1 at 23°C. If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. Calculate the half-life of the reaction when the initial concentration of I is 0.60 M and when the initial concentration of I is 0.42 M.