TReview lopicS] TRelerences Nitrogen dioxide, NO2, decomposes upon heating to form nitric oxide and oxygen according to the following equation: 2NO2 (9) → 2NO(9) + O2 (g) At the beginning of an experiment, the concentration of nitrogen dioxide in a reaction vessel was 0.1103 mol/L. After 69.0 s, the concentration decreased to 0.1067 mol/L. What is the average rate of decomposition of NO2 during this time interval in mol/(L-s)? Average rate = mol/(L-s)
TReview lopicS] TRelerences Nitrogen dioxide, NO2, decomposes upon heating to form nitric oxide and oxygen according to the following equation: 2NO2 (9) → 2NO(9) + O2 (g) At the beginning of an experiment, the concentration of nitrogen dioxide in a reaction vessel was 0.1103 mol/L. After 69.0 s, the concentration decreased to 0.1067 mol/L. What is the average rate of decomposition of NO2 during this time interval in mol/(L-s)? Average rate = mol/(L-s)
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.87PAE
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Step 1
given
Initial concentration of nitrogen dioxide (NO2)
= 0.1103 mol/L
Final concentration of NO2
= 0.1076 mol/L
Time taken = 65.0 s
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