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The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H,-I, + 2 HCI Experiment [ICI],, M [H,],, M Initial Rate, M s"! 1 0.367 0.226 3.58×10-2 0.734 0.226 7.16×10-2 0.367 0.451 0.143 4 0.734 0.451 0.285 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1.

The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H,-I, + 2 HCI Experiment [ICI],, M [H,],, M Initial Rate, M s"! 1 0.367 0.226 3.58×10-2 0.734 0.226 7.16×10-2 0.367 0.451 0.143 4 0.734 0.451 0.285 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1.

Introduction to Chemical Engineering Thermodynamics
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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The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI+ H2- →I2 + 2 HCl Experiment [ICI],, M [H,]o, M Initial Rate, M s 1 0.367 0.226 3.58×10-2 2 0.734 0.226 7.16×10-2 3 0.367 0.451 0.143 4 0.734 0.451 0.285 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1.
Transcribed Image Text:The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI+ H2- →I2 + 2 HCl Experiment [ICI],, M [H,]o, M Initial Rate, M s 1 0.367 0.226 3.58×10-2 2 0.734 0.226 7.16×10-2 3 0.367 0.451 0.143 4 0.734 0.451 0.285 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1.
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