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The reaction 2NO(g) + Cl₂ (g) → 2NOC1(g) was studied at -10°C. The following results were obtained where A[C1₂] At [C1z]o Rate = [NO]o (mol/L) (mol/L) (mol/L.min) 0.12 0.12 0.31 0.12 0.24 0.62 0.24 0.24 2.49 Initial Rate a What is the rate law? (Use k for the rate constant. ) Rate = a The reaction of NO₂ (g) and CO(g) is thought to occur in two steps: Step 1 Slow NO₂(g) + NO2(g) → NO(g) + NO3 (9) Step 2 Fast NO3(g) + CO(g) → NO2 (g) + CO₂(g) Add the elementary steps to give the overall, stoichiometric reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

The reaction 2NO(g) + Cl₂ (g) → 2NOC1(g) was studied at -10°C. The following results were obtained where A[C1₂] At [C1z]o Rate = [NO]o (mol/L) (mol/L) (mol/L.min) 0.12 0.12 0.31 0.12 0.24 0.62 0.24 0.24 2.49 Initial Rate a What is the rate law? (Use k for the rate constant. ) Rate = a The reaction of NO₂ (g) and CO(g) is thought to occur in two steps: Step 1 Slow NO₂(g) + NO2(g) → NO(g) + NO3 (9) Step 2 Fast NO3(g) + CO(g) → NO2 (g) + CO₂(g) Add the elementary steps to give the overall, stoichiometric reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter16: Reaction Rates
Section: Chapter Questions
Problem 81A
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The reaction 2NO(g) + Cl₂ (g) → 2NOC1(g) was studied at -10°C. The following results were obtained where A[C1₂] At [C1z]o Rate = [NO]o (mol/L) (mol/L) (mol/L.min) 0.12 0.12 0.31 0.12 0.24 0.62 0.24 0.24 2.49 Initial Rate a What is the rate law? (Use k for the rate constant. ) Rate =
Transcribed Image Text:The reaction 2NO(g) + Cl₂ (g) → 2NOC1(g) was studied at -10°C. The following results were obtained where A[C1₂] At [C1z]o Rate = [NO]o (mol/L) (mol/L) (mol/L.min) 0.12 0.12 0.31 0.12 0.24 0.62 0.24 0.24 2.49 Initial Rate a What is the rate law? (Use k for the rate constant. ) Rate =
a The reaction of NO₂ (g) and CO(g) is thought to occur in two steps: Step 1 Slow NO₂(g) + NO2(g) → NO(g) + NO3 (9) Step 2 Fast NO3(g) + CO(g) → NO2 (g) + CO₂(g) Add the elementary steps to give the overall, stoichiometric reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
Transcribed Image Text:a The reaction of NO₂ (g) and CO(g) is thought to occur in two steps: Step 1 Slow NO₂(g) + NO2(g) → NO(g) + NO3 (9) Step 2 Fast NO3(g) + CO(g) → NO2 (g) + CO₂(g) Add the elementary steps to give the overall, stoichiometric reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
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