Rates of chemical reaction Nitrogen dioxide, NO2, decomposes upon heating to form nitric oxide and oxygen according to the equation 2 NO2 (g) → 2 NO (g) + O2 (g) At the beginning of an experiment, the concentration of nitrogen dioxide in a reaction vessel was 0.1213 M. After 55 seconds the concentration decreased to 0.1105 M. What is the average rate of decomposition of NO2 during this time interval in M/s?
Rates of chemical reaction Nitrogen dioxide, NO2, decomposes upon heating to form nitric oxide and oxygen according to the equation 2 NO2 (g) → 2 NO (g) + O2 (g) At the beginning of an experiment, the concentration of nitrogen dioxide in a reaction vessel was 0.1213 M. After 55 seconds the concentration decreased to 0.1105 M. What is the average rate of decomposition of NO2 during this time interval in M/s?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
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 24PS: Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is...
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Nitrogen dioxide, NO2, decomposes upon heating to form nitric oxide and oxygen according to the equation 2 NO2 (g) → 2 NO (g) + O2 (g)
At the beginning of an experiment, the concentration of nitrogen dioxide in a reaction vessel was 0.1213 M. After 55 seconds the concentration decreased to 0.1105 M. What is the average rate of decomposition of NO2 during this time interval in M/s?
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