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K12.90 Rate constants for the reaction NO2(g) + CO(g) – NO(g) + CO2(g) are 1.3 M-1s at 700 K and 23.0 M-1s-1 -> at 800 K. (a) What is the value of the activation energy in kJ/mol? (b) What is the rate constant at 750 K?

K12.90 Rate constants for the reaction NO2(g) + CO(g) – NO(g) + CO2(g) are 1.3 M-1s at 700 K and 23.0 M-1s-1 -> at 800 K. (a) What is the value of the activation energy in kJ/mol? (b) What is the rate constant at 750 K?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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K12.90 Rate constants for the reaction NO2(g) + CO(g) – NO(g) + CO2(g) are 1.3 M-1s at 700 K and 23.0 M-1s-1 -> at 800 K. (a) What is the value of the activation energy in kJ/mol? (b) What is the rate constant at 750 K?
Transcribed Image Text:K12.90 Rate constants for the reaction NO2(g) + CO(g) – NO(g) + CO2(g) are 1.3 M-1s at 700 K and 23.0 M-1s-1 -> at 800 K. (a) What is the value of the activation energy in kJ/mol? (b) What is the rate constant at 750 K?
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