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3. Determine the full rate law (via the method of initial rates), the overall order of reaction, and rate constant (in appropriate units to one decimal place) for the following reaction and provided experimental data. 2NO(g) + Cl₂(g) → 2NOC1(g) Trial NO (M) Cl₂ (M) Rate (Ms¯¹) 1 2 3 0.10 0.10 0.15 0.10 0.15 0.10 0.00300 0.00450 0.00675 A: 3rd order; k = 3.0

3. Determine the full rate law (via the method of initial rates), the overall order of reaction, and rate constant (in appropriate units to one decimal place) for the following reaction and provided experimental data. 2NO(g) + Cl₂(g) → 2NOC1(g) Trial NO (M) Cl₂ (M) Rate (Ms¯¹) 1 2 3 0.10 0.10 0.15 0.10 0.15 0.10 0.00300 0.00450 0.00675 A: 3rd order; k = 3.0

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Dinitrogen pentoxide, N2O5, decomposes via the following reaction
3. Determine the full rate law (via the method of initial rates), the overall order of reaction, and rate constant (in appropriate units to one decimal place) for the following reaction and provided experimental data. 2NO(g) + Cl₂(g) → 2NOCI(g) Trial NO (M) Cl₂ (M) 1 2 0.10 0.10 0.15 0.10 0.15 0.10 s-¹) Rate (M s 0.00300 0.00450 0.00675 18.0 4 (4) A: 3rd order; k = 3.0
Transcribed Image Text:3. Determine the full rate law (via the method of initial rates), the overall order of reaction, and rate constant (in appropriate units to one decimal place) for the following reaction and provided experimental data. 2NO(g) + Cl₂(g) → 2NOCI(g) Trial NO (M) Cl₂ (M) 1 2 0.10 0.10 0.15 0.10 0.15 0.10 s-¹) Rate (M s 0.00300 0.00450 0.00675 18.0 4 (4) A: 3rd order; k = 3.0
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