In the 1890s, experiments on the reaction H2(g) + 12(g) → 2 HI (g) showed that the rate law is first order in each of the reactants and second order overall. It was thought to be an elementary reaction. New experiments in the 1960s led to proposal of the following mechanism: 1) 2→21 2) 21→ I2 3) I+H2 → IH2 4) I+ IH2 → 2 HI rate constant k] rate constant k2 rate constant k3 rate constant k4 Assume that reactions 1 and 2 are much faster than reactions 3 and 4 and therefore yield a pre-equilibrium, and that the steady-state assumption applies to IH2, to obtain the overall rate law from this mechanism.
In the 1890s, experiments on the reaction H2(g) + 12(g) → 2 HI (g) showed that the rate law is first order in each of the reactants and second order overall. It was thought to be an elementary reaction. New experiments in the 1960s led to proposal of the following mechanism: 1) 2→21 2) 21→ I2 3) I+H2 → IH2 4) I+ IH2 → 2 HI rate constant k] rate constant k2 rate constant k3 rate constant k4 Assume that reactions 1 and 2 are much faster than reactions 3 and 4 and therefore yield a pre-equilibrium, and that the steady-state assumption applies to IH2, to obtain the overall rate law from this mechanism.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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This is regarding rate laws. Please help with steps and explanation
Transcribed Image Text:In the 1890s, experiments on the reaction H₂(g) + I₂(g) → 2 HI (g) showed that the rate law is first order in each of the reactants and second order overall. It was thought to be an elementary reaction. New experiments in the 1960s led to the proposal of the following mechanism:
1) I₂ → 2 I
- Rate constant: k₁
2) 2 I → I₂
- Rate constant: k₂
3) I + H₂ → IH₂
- Rate constant: k₃
4) I + IH₂ → 2 HI
- Rate constant: k₄
Assume that reactions 1 and 2 are much faster than reactions 3 and 4 and therefore yield a pre-equilibrium, and that the steady-state assumption applies to IH₂, to obtain the overall rate law from this mechanism.
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