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he decomposition of ozone in the upper atmosphere to dioxygen occurs - he first step is a fast reversible step and the second is a slow reaction between an ozone molecule: Step 1: Step 2: O3(g) = 02(g) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, rea Slow

he decomposition of ozone in the upper atmosphere to dioxygen occurs - he first step is a fast reversible step and the second is a slow reaction between an ozone molecule: Step 1: Step 2: O3(g) = 02(g) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, rea Slow

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
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O 11. The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism. The first step is a fast reversible step and the second is a slow reaction between an oxygen atom and an ozone molecule: Step 1: Step 2: O3(g) = 02(8) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, reaction Slow a. Which is the rate determining step? b. Write the rate equation for the rate-determining step. Write the rate equation for the overall reaction. с. The rate equation for the reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: 12. NO2(g) + CO(g) → NO(g) + CO2(g) The following data were collected at 125°C:e Experiment 1 Experiment 2 Experiment 3 Initial [NO2] mol L 5.0 x 104 5.0 x 104 1.5 x 10-3 Initial [CO] mol L- 1.6 x 10-2 3.2 x 102 3.2 x 10-2 Initial rate mol L'min 1.7 x 10-7 1.7 x 10-7 1.5 x 10-6 What is the order with respect to NO2? b. What is the order with respect to CO? c. What is the overall order of the reaction? d. Write the rate equation. e. How do you know this is not a single step reaction? a. oil boniside stow ssb gniwolkle
Transcribed Image Text:O 11. The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism. The first step is a fast reversible step and the second is a slow reaction between an oxygen atom and an ozone molecule: Step 1: Step 2: O3(g) = 02(8) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, reaction Slow a. Which is the rate determining step? b. Write the rate equation for the rate-determining step. Write the rate equation for the overall reaction. с. The rate equation for the reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: 12. NO2(g) + CO(g) → NO(g) + CO2(g) The following data were collected at 125°C:e Experiment 1 Experiment 2 Experiment 3 Initial [NO2] mol L 5.0 x 104 5.0 x 104 1.5 x 10-3 Initial [CO] mol L- 1.6 x 10-2 3.2 x 102 3.2 x 10-2 Initial rate mol L'min 1.7 x 10-7 1.7 x 10-7 1.5 x 10-6 What is the order with respect to NO2? b. What is the order with respect to CO? c. What is the overall order of the reaction? d. Write the rate equation. e. How do you know this is not a single step reaction? a. oil boniside stow ssb gniwolkle
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