At high concentrations of [H2] the observed rate law is found to change to the form: Rate = k[NO]? i.e. the rate becomes independent of [H2]. Assess whether the two step mechanism that you showed to be plausible at lower[H2] concentrations in the pre- problem can also explain this additional data. Reexamine the mechanism in the Pre-recitation Problem: 2NO + H2 → O + H20 + N2 slow ki 0 + H2 → H2O k2 Write the forward rates for both steps.

At high concentrations of [H2] the observed rate law is found to change to the form: Rate = k[NO]? i.e. the rate becomes independent of [H2]. Assess whether the two step mechanism that you showed to be plausible at lower[H2] concentrations in the pre- problem can also explain this additional data. Reexamine the mechanism in the Pre-recitation Problem: 2NO + H2 → O + H20 + N2 slow ki 0 + H2 → H2O k2 Write the forward rates for both steps.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.3: Rate Law And Order Of Reactions

Problem 11.4PSP

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