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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Question

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.)

____________

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions