+ O2--> OH + O has a rate constant = 4.7 * 10-7 M-1s-1 at 1000K. The activiation energy required = 66.5 kj/mol. Calculate the rate constant at 2000K. Plot the concentration vs time that corresponds to your answer.
+ O2--> OH + O has a rate constant = 4.7 * 10-7 M-1s-1 at 1000K. The activiation energy required = 66.5 kj/mol. Calculate the rate constant at 2000K. Plot the concentration vs time that corresponds to your answer.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 68QAP: For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at 25C...
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H + O2--> OH + O has a rate constant = 4.7 * 10-7 M-1s-1 at 1000K. The activiation energy required = 66.5 kj/mol.
Calculate the rate constant at 2000K.
Plot the concentration vs time that corresponds to your answer.
*Please help exlain why this is the correct plot. I am confused since there are three different ways to plot them:
- [A] vs. Time
- ln[A] vs. Time
- 1/[A] vs. time
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