The rate of the elementary reaction O₂+ H₂ → OH + OH has been studied as a function of temperature between 803 and 1250 K. The following data were obtained for the rate constant, k: Temperature (K) k, 803 A = L mol-s 892 981 L mol-s 2.75 x 10-1 4.18 x 10⁰ 3.87 x 10¹ 2.48 x 10² 1070 Calculate the activation energy of this reaction. E₁ = kJ/mol Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.
The rate of the elementary reaction O₂+ H₂ → OH + OH has been studied as a function of temperature between 803 and 1250 K. The following data were obtained for the rate constant, k: Temperature (K) k, 803 A = L mol-s 892 981 L mol-s 2.75 x 10-1 4.18 x 10⁰ 3.87 x 10¹ 2.48 x 10² 1070 Calculate the activation energy of this reaction. E₁ = kJ/mol Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter12: Kinetics
Section: Chapter Questions
Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
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![The rate of the elementary reaction
O2+ H₂ → OH + OH
has been studied as a function of temperature between 803 and 1250 K. The following data were
obtained for the rate constant, k:
Temperature (K) k,
E
803
A =
L
mol-s
892
981
1070
Calculate the activation energy of this reaction.
kJ/mol
Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate
constant.
mol-s
Submit Answer
2.75 x 10-1
4.18 x 10⁰
3.87 x 10¹
2.48 x 10²
Try Another Version
2 item attempts remaining](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F91786a22-2c5c-41a2-a98f-fcd31791308b%2F10d5535a-01eb-4a02-847a-5839811bf820%2Ftpfqdhd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The rate of the elementary reaction
O2+ H₂ → OH + OH
has been studied as a function of temperature between 803 and 1250 K. The following data were
obtained for the rate constant, k:
Temperature (K) k,
E
803
A =
L
mol-s
892
981
1070
Calculate the activation energy of this reaction.
kJ/mol
Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate
constant.
mol-s
Submit Answer
2.75 x 10-1
4.18 x 10⁰
3.87 x 10¹
2.48 x 10²
Try Another Version
2 item attempts remaining
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