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The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g) + ½ O₂(g) is second order in NO2. In one experiment, when the initial concentration of NO₂ was 0.136 M, the concentration of NO2 dropped to 3.62 x 10-2 M after 28.7 seconds had passed. Based on these data, the rate constant for the reaction is M¹ s²-¹.

The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g) + ½ O₂(g) is second order in NO2. In one experiment, when the initial concentration of NO₂ was 0.136 M, the concentration of NO2 dropped to 3.62 x 10-2 M after 28.7 seconds had passed. Based on these data, the rate constant for the reaction is M¹ s²-¹.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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 21PS: At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an...
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Tbed image Text: The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g) + ½/2O₂(g) is second order in NO2. In one experiment, when the initial concentration of NO2 was 0.136 M, the concentration of NO2 dropped to 3.62 x 10-2 M after 28.7 seconds had passed. Based on these data, the rate constant for the reaction is I Use the ices to access important M-¹ s-¹. destion. The ergy for the gas phase isoff zation JL 1
Transcribed Image Text:Tbed image Text: The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g) + ½/2O₂(g) is second order in NO2. In one experiment, when the initial concentration of NO2 was 0.136 M, the concentration of NO2 dropped to 3.62 x 10-2 M after 28.7 seconds had passed. Based on these data, the rate constant for the reaction is I Use the ices to access important M-¹ s-¹. destion. The ergy for the gas phase isoff zation JL 1
Consider the combustion of ethane: 2C2H6 (9) +702(g) → 4 CO₂ (g) + 6H₂O(g) If the ethane is burning at the rate of 0.8 mol/L x s, at what rates are CO₂ and H₂O being produced? CO₂ = H₂O = mol/L x s mol/L x s
Transcribed Image Text:Consider the combustion of ethane: 2C2H6 (9) +702(g) → 4 CO₂ (g) + 6H₂O(g) If the ethane is burning at the rate of 0.8 mol/L x s, at what rates are CO₂ and H₂O being produced? CO₂ = H₂O = mol/L x s mol/L x s
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