The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C,2H22011 + H,0 - C,H20, + C,H206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate - k [C,,H2,o,,) (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, I.e. they are isomers.) (a) In neutral solution, k- 1.8 x 10-11 s at 26°C and 8.5x 10-11s- at 37°C. Determine the activation energy (In kJ/mol), the frequency factor (in s), and the rate constant (In s) for this equation at 48°C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (Enter unrounded values.) activation energy 108 v k/mol frequency factor rate constant x s1 (b) When a solution of sucrose with an Initlal concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40 x 10- M. How long (in s) will it take the solution to reach equilibrium sucrose at equllibrium is so low, assume that the reaction is Irreversible. (Enter an unrounded value.) 26°C in the absence of a catalyst? Because the concentration of
The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C,2H22011 + H,0 - C,H20, + C,H206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate - k [C,,H2,o,,) (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, I.e. they are isomers.) (a) In neutral solution, k- 1.8 x 10-11 s at 26°C and 8.5x 10-11s- at 37°C. Determine the activation energy (In kJ/mol), the frequency factor (in s), and the rate constant (In s) for this equation at 48°C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (Enter unrounded values.) activation energy 108 v k/mol frequency factor rate constant x s1 (b) When a solution of sucrose with an Initlal concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40 x 10- M. How long (in s) will it take the solution to reach equilibrium sucrose at equllibrium is so low, assume that the reaction is Irreversible. (Enter an unrounded value.) 26°C in the absence of a catalyst? Because the concentration of
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 hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows.
C12H22011 + H20 → C;H1206 + CGH12°6
This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C, ,H,,0,,] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are
22
isomers.)
s-1
at 26°C and 8.5x10-11 s at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s-), and the rate constant (ins-) for this equation at 48°C (assuming the kinetics remain consistent with the
(a)
In neutral solution, k
1.8×10-11
Arrhenius equation at this temperature). (Enter unrounded values.)
%3D
activation energy
108
kJ/mol
frequency factor
s-1
rate constant
X s-1
When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10- M. How long (in s) will it take the solution to reach equilibrium at 26°C in the absence of a catalyst? Because the concentration of
(b)
sucrose at equilibrium is so low, assume that the reaction is irreversible. (Enter an unrounded value.)
(c)
Why does assuming that the reaction is irreversible simplify the calculation in part (h)2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1593f45e-4da7-40d4-bc81-735ecba0bfae%2F05b03698-4889-4c35-9b6b-f88100935877%2Fg1xdhij_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows.
C12H22011 + H20 → C;H1206 + CGH12°6
This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C, ,H,,0,,] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are
22
isomers.)
s-1
at 26°C and 8.5x10-11 s at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s-), and the rate constant (ins-) for this equation at 48°C (assuming the kinetics remain consistent with the
(a)
In neutral solution, k
1.8×10-11
Arrhenius equation at this temperature). (Enter unrounded values.)
%3D
activation energy
108
kJ/mol
frequency factor
s-1
rate constant
X s-1
When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10- M. How long (in s) will it take the solution to reach equilibrium at 26°C in the absence of a catalyst? Because the concentration of
(b)
sucrose at equilibrium is so low, assume that the reaction is irreversible. (Enter an unrounded value.)
(c)
Why does assuming that the reaction is irreversible simplify the calculation in part (h)2
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