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The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures: Determine the activation energy graphically. Go k(M1·s)| T(°C) 1.87 × 10-3| 600 0.0113 650 0.0569 700 0.244 750 x 10 kJ/mol (Enter your answer in scientific notation.)

The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures: Determine the activation energy graphically. Go k(M1·s)| T(°C) 1.87 × 10-3| 600 0.0113 650 0.0569 700 0.244 750 x 10 kJ/mol (Enter your answer in scientific notation.)

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.55PAE: The following rate constants were obtained in an experiment in which the decomposition of gaseous...
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Be sure to answer all parts. The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures: Determine the activation energy graphically. Gr k(M'·s) | T(°C) 1.87 × 10 3 600 0.0113 650 0.0569 700 0.244 750 × 10 kJ/mol (Enter your answer in scientific notation.)
Transcribed Image Text:Be sure to answer all parts. The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures: Determine the activation energy graphically. Gr k(M'·s) | T(°C) 1.87 × 10 3 600 0.0113 650 0.0569 700 0.244 750 × 10 kJ/mol (Enter your answer in scientific notation.)
Expert Solution
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The rate constant with respect to temperature was explained by Arrhenius by using equation 

lnK = (- Ea / RT) + lnA 

Ea = activation energy kj / mol

R = 8.314 j/ mol k

A = pre exponential factor

K = rate constant

T = temperature in Kelvin

 

 

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