To what temperature would the reaction below need to be heated to have a rate constant of 2.475e-3 M-1/2s-1 if the rate constant was 1.0500e-3 M-1/2s-1 at 486.00°C and the activation energy was 207.000 kJ/mol? CH3CHO(g) ↔ CH4(g) + CO(g) 767.87°C 494.72°C 477.36°C 506.38°C
To what temperature would the reaction below need to be heated to have a rate constant of 2.475e-3 M-1/2s-1 if the rate constant was 1.0500e-3 M-1/2s-1 at 486.00°C and the activation energy was 207.000 kJ/mol? CH3CHO(g) ↔ CH4(g) + CO(g) 767.87°C 494.72°C 477.36°C 506.38°C
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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
Section: Chapter Questions
Problem 23PS: The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction (Figure...
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To what temperature would the reaction below need to be heated to have a rate constant of 2.475e-3 M-1/2s-1 if the rate constant was 1.0500e-3 M-1/2s-1 at 486.00°C and the activation energy was 207.000 kJ/mol?
CH3CHO(g) ↔ CH4(g) + CO(g)
767.87°C
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|
494.72°C
|
|
477.36°C
|
|
506.38°C
|
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