The rate constant for the second-order reaction 2NOBR() – 2NOg) + Br2g) is 0.80/M · s at 10°C. (a) Starting with a concentration of 0.086 M, calculate the concentration of NOB after 22 s. (b) Calculate the half-lives when [NOB1]o = 0.072 M and [NOB1]o = 0.054 M.
The rate constant for the second-order reaction 2NOBR() – 2NOg) + Br2g) is 0.80/M · s at 10°C. (a) Starting with a concentration of 0.086 M, calculate the concentration of NOB after 22 s. (b) Calculate the half-lives when [NOB1]o = 0.072 M and [NOB1]o = 0.054 M.
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Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.107QP
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![The rate constant for the second-order reaction 2NOBrg) → 2NOg) + Br2g) is
0.80/M · s at 10°C.
(a) Starting with a concentration of 0.086 M, calculate the concentration of NOBr after 22 s.
(b) Calculate the half-lives when [NOB1]o = 0.072 M and [NOB1]o = 0.054 M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F686755b6-e64f-45c8-968d-094b90cdaeb3%2F6dd8464f-2858-45a6-8cee-e6b56bd7f9e7%2Fubfxtro_processed.png&w=3840&q=75)
Transcribed Image Text:The rate constant for the second-order reaction 2NOBrg) → 2NOg) + Br2g) is
0.80/M · s at 10°C.
(a) Starting with a concentration of 0.086 M, calculate the concentration of NOBr after 22 s.
(b) Calculate the half-lives when [NOB1]o = 0.072 M and [NOB1]o = 0.054 M.
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