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A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(g) + O₂(g) → NO₂ (9) ->> Conc. NO, mol/L Exp. 1 1.2 x 10-2 Exp. 2 1.2 x 10-² Exp. 3 2.4 x 10-2 Exp. 4 0.17 Conc. 02, mol/L 3.6 x 10-2 7.2 x 10-2 0.14 9.6 × 10³ Initial Rate 9.3 x 10 mol/(L-s) 1.9 x 103 mol/(L-B) 1.4 x 102 mol/(L-s) ? What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law

A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(g) + O₂(g) → NO₂ (9) ->> Conc. NO, mol/L Exp. 1 1.2 x 10-2 Exp. 2 1.2 x 10-² Exp. 3 2.4 x 10-2 Exp. 4 0.17 Conc. 02, mol/L 3.6 x 10-2 7.2 x 10-2 0.14 9.6 × 10³ Initial Rate 9.3 x 10 mol/(L-s) 1.9 x 103 mol/(L-B) 1.4 x 102 mol/(L-s) ? What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 79QRT
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A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(g) + O₂(g) → NO₂ (9) Conc. NO, mol/L Exp. 1 1.2 x 10-2 Exp. 2 1.2 x 10-² Exp. 3 2.4 x 10-2 Exp. 4 0.17 Conc. 02, mol/L Initial Rate 3.6 x 10-2 7.2 x 10-2 0.14 9.6 × 10 9.3 x 10 mol/(L-s) 1.9 x 103 mol/(L-B) 1.4 x 102 mol/(L-s) ? What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law
Transcribed Image Text:A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(g) + O₂(g) → NO₂ (9) Conc. NO, mol/L Exp. 1 1.2 x 10-2 Exp. 2 1.2 x 10-² Exp. 3 2.4 x 10-2 Exp. 4 0.17 Conc. 02, mol/L Initial Rate 3.6 x 10-2 7.2 x 10-2 0.14 9.6 × 10 9.3 x 10 mol/(L-s) 1.9 x 103 mol/(L-B) 1.4 x 102 mol/(L-s) ? What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law
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