Nitrogen dioxide decomposed upon heating to form nitric oxide and oxygen according to the following equation 2NO2(g) -> 2NO(g) +O2(g) at the beginning of an experiment the concentration of nitrogen dioxide in a reaction vessel was .1103 mol/L. After 64.0 s the concentration decreased to 0.1088mol/L. What is the average rate of decomposition of NO2 during this time interval in mol(L•s) average rate = blank
Nitrogen dioxide decomposed upon heating to form nitric oxide and oxygen according to the following equation 2NO2(g) -> 2NO(g) +O2(g) at the beginning of an experiment the concentration of nitrogen dioxide in a reaction vessel was .1103 mol/L. After 64.0 s the concentration decreased to 0.1088mol/L. What is the average rate of decomposition of NO2 during this time interval in mol(L•s) average rate = blank
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 decomposed upon heating to form nitric oxide and oxygen according to the following equation
2NO2(g) -> 2NO(g) +O2(g)
at the beginning of an experiment the concentration of nitrogen dioxide in a reaction vessel was .1103 mol/L. After 64.0 s the concentration decreased to 0.1088mol/L. What is the average rate of decomposition of NO2 during this time interval in mol(L•s)
average rate = blank
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