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Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k, and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law.

Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k, and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law.

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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just need help with d and e please

Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
Transcribed Image Text:Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
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