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At the start of the reaction, the concentration of YOI is equal to 5.142 M. After 118.0 seconds, its concentration was reduced to 2.361 M. Meanwhile, another run of the same reaction but with 3.789 M [YOI]0 showed that after 110.0 seconds, a 1.350 M decrease in concentration of YOI was observed. Based on these: 1. Estimate the order of the reaction. 2. How much YOI will be consumed if a run with [YOI]0 = 1.234 M is allowed to form MIYA for 4.00 minutes.

At the start of the reaction, the concentration of YOI is equal to 5.142 M. After 118.0 seconds, its concentration was reduced to 2.361 M. Meanwhile, another run of the same reaction but with 3.789 M [YOI]0 showed that after 110.0 seconds, a 1.350 M decrease in concentration of YOI was observed. Based on these: 1. Estimate the order of the reaction. 2. How much YOI will be consumed if a run with [YOI]0 = 1.234 M is allowed to form MIYA for 4.00 minutes.

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 11.40PAE: In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the...
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At the start of the reaction, the concentration of YOI is equal to 5.142 M. After 118.0 seconds, its concentration was reduced to 2.361 M. Meanwhile, another run of the same reaction but with 3.789 M [YOI]0 showed that after 110.0 seconds, a 1.350 M decrease in concentration of YOI was observed. Based on these:

1. Estimate the order of the reaction.
2. How much YOI will be consumed if a run with [YOI]0 = 1.234 M is allowed to form MIYA for 4.00 minutes.

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In the amount of YOI consumed, my answer seems to be different from the solution. My answer is 0.319 M and the solution gave an answer of 0.2525 M. Could you help me check if 0.2525 M is really the answer? Thank you.

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