The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22O11 + H2O → C6H12O6 + C6H12O6 This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C12H22O11] (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 ✕ 10−11 s−1 at 26°C and 8.5 ✕ 10−11 s−1 at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s−1), and the rate constant (in s−1) for this equation at 48°C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (Enter unrounded values.) FREQUENCY FACTOR??_____ RATE CONSTANT?? _ (b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40 ✕ 10−7 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 sucrose at equilibrium is so low, assume that the reaction is irreversible. (Enter an unrounded value.) ________

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 65E: The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6...

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The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows.

C₁₂H₂₂O₁₁ + H₂O → C₆H₁₂O₆ + C₆H₁₂O₆

This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C₁₂H₂₂O₁₁] (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 ✕ 10⁻¹¹ s⁻¹ at 26°C and 8.5 ✕ 10⁻¹¹ s⁻¹ at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s⁻¹), and the rate constant (in s⁻¹) for this equation at 48°C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (Enter unrounded values.)

FREQUENCY FACTOR??_________

RATE CONSTANT?? _________

(b)

When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40 ✕ 10⁻⁷ 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 sucrose at equilibrium is so low, assume that the reaction is irreversible. (Enter an unrounded value.)

____________

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