Suppose the experiment is run with these initial concentrations, and the disappearance of purple coloration is determined by measuring the absorbance of 590 nm light using a spectrophotometer: [CV*], = 5.0 x 10³M [OH], = 0.88 M The observed rate constant, k’ , was determined graphically to be 0.046 minª. (a) Re-write the rate law using k' and the pseudo-first order assumption: Rate = (b) Calculate the overall rate constant, k.
Suppose the experiment is run with these initial concentrations, and the disappearance of purple coloration is determined by measuring the absorbance of 590 nm light using a spectrophotometer: [CV*], = 5.0 x 10³M [OH], = 0.88 M The observed rate constant, k’ , was determined graphically to be 0.046 minª. (a) Re-write the rate law using k' and the pseudo-first order assumption: Rate = (b) Calculate the overall rate constant, k.
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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![N(CH32
N(CH3)2
он
-N(CH3)2 + OH .
-N(CH2
N(CH,2
N(CH2
CV (aq)
+ OH- →
→ CVOH(aq)
Violet
Colorless
7. The purple dye, Crystal Violet (CV*) can be turned colorless by reaction with hydroxide ions (basic
solution). When studying the kinetics of the reaction, which is sterically hindered, it is common to use a
large excess of one reactant while observing changes in the other. This reaction has the following rate
law:
rate = k[CV*][OH]
Suppose the experiment is run with these initial concentrations, and the disappearance of purple coloration
is determined by measuring the absorbance of 590 nm light using a spectrophotometer:
[CV*], = 5.0 x 10$M [OH]], = 0.88 M
The observed rate constant, k’ , was determined graphically to be 0.046 min!.
(a) Re-write the rate law using k' and the pseudo-first order assumption:
Rate =
(b) Calculate the overall rate constant, k.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b1d6994-83c0-472b-a60c-05f27149766f%2F5644cc70-999b-4096-9ef4-78b0fc37418d%2Fnsm6fts_processed.png&w=3840&q=75)
Transcribed Image Text:N(CH32
N(CH3)2
он
-N(CH3)2 + OH .
-N(CH2
N(CH,2
N(CH2
CV (aq)
+ OH- →
→ CVOH(aq)
Violet
Colorless
7. The purple dye, Crystal Violet (CV*) can be turned colorless by reaction with hydroxide ions (basic
solution). When studying the kinetics of the reaction, which is sterically hindered, it is common to use a
large excess of one reactant while observing changes in the other. This reaction has the following rate
law:
rate = k[CV*][OH]
Suppose the experiment is run with these initial concentrations, and the disappearance of purple coloration
is determined by measuring the absorbance of 590 nm light using a spectrophotometer:
[CV*], = 5.0 x 10$M [OH]], = 0.88 M
The observed rate constant, k’ , was determined graphically to be 0.046 min!.
(a) Re-write the rate law using k' and the pseudo-first order assumption:
Rate =
(b) Calculate the overall rate constant, k.
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