Given the following mechanism: 2NO N202 step 1 (fast, call the rate constants k1 and k-1) N202+H2N20 + H20 (slow, call the rate constant for this step k2) step 2 (call the rate constant for this step ka) N20 H2 N2 H20 step 3 Determine the overall reaction. а. b. Are there any intermediates in this reaction mechanism? If so, which one(s)? Determine the rate law. Intermediates may not appear in rate laws. Use the equilibrium с. expression to write the rate law only in terms of [reactants]. What is the overall order of the reactions? d. What is the molecularity of the rate determining step? е.

Given the following mechanism: 2NO N202 step 1 (fast, call the rate constants k1 and k-1) N202+H2N20 + H20 (slow, call the rate constant for this step k2) step 2 (call the rate constant for this step ka) N20 H2 N2 H20 step 3 Determine the overall reaction. а. b. Are there any intermediates in this reaction mechanism? If so, which one(s)? Determine the rate law. Intermediates may not appear in rate laws. Use the equilibrium с. expression to write the rate law only in terms of [reactants]. What is the overall order of the reactions? d. What is the molecularity of the rate determining step? е.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section14.6: Reaction Mechanisms

Problem 1RC: The rate equation for a reaction A + B C was determined by experiment to be Rate = k[A][B]. From...

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