The rate constant for the following second-order reaction is 0.80 (M.s) at 10.0 °C. 2NOBr(g) 2NO(g) + Br₂ (g) Calculate the half-life, in seconds, when [NOBr] = 0.116 M. Round your answer to 2 significant digits.
The rate constant for the following second-order reaction is 0.80 (M.s) at 10.0 °C. 2NOBr(g) 2NO(g) + Br₂ (g) Calculate the half-life, in seconds, when [NOBr] = 0.116 M. Round your answer to 2 significant digits.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.4: Concentration-time Relationships: Integrated Rate Laws
Problem 14.8CYU: The catalyzed decomposition of hydrogen peroxide is first-order in [H2O2]. It was found that the...
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![The rate constant for the following second-order reaction is
S
2NOBr(g) → 2NO(g) + Br₂ (g)
Calculate the half-life, in seconds, when [NOBr] = 0.116 M. Round your answer to 2 significant digits.
x10
x
0.80
(M.s)
S
at 10.0 °C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F287b9249-0891-4268-81e8-44cc307be217%2F4495f1e1-4ac7-42e8-8a76-95360d1bc480%2Fmumyqye_processed.png&w=3840&q=75)
Transcribed Image Text:The rate constant for the following second-order reaction is
S
2NOBr(g) → 2NO(g) + Br₂ (g)
Calculate the half-life, in seconds, when [NOBr] = 0.116 M. Round your answer to 2 significant digits.
x10
x
0.80
(M.s)
S
at 10.0 °C.
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