Homework Help is Here – Start Your Trial Now!
Science
Chemistry
3. Sucrose decomposes in aqueous solution into a mixture of two sugars, glucose and fructose. C„H,„0, (aq) + H,0(1) I C,H,„O,(aq) + C,H,„O,(aq) The observed initial rates of decomposition of sucrose at two different initial sucrose concentrations at 25°C are: Rate ( M sec ") [Sucrose] 8.5 X 10 -3 1.71 X 102 0.1 0.2

3. Sucrose decomposes in aqueous solution into a mixture of two sugars, glucose and fructose. C„H,„0, (aq) + H,0(1) I C,H,„O,(aq) + C,H,„O,(aq) The observed initial rates of decomposition of sucrose at two different initial sucrose concentrations at 25°C are: Rate ( M sec ") [Sucrose] 8.5 X 10 -3 1.71 X 102 0.1 0.2

Chemistry
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
icon
Related questions
Question
3. Sucrose decomposes in aqueous solution into a mixture of two sugars, glucose and fructose. C„H„0, (aq) + H,0(1) I C,H,,0,(aq) + C,H,„O,(aq) The observed initial rates of decomposition of sucrose at two different initial sucrose concentrations at 25°C are: Rate ( M sec ') [Sucrose] 0.1 8.5 X 10 -3 1.71 X 102 0.2 Find the dependence of the reaction rate on the concentration of sucrose and compute the rate constant for the reaction.
Transcribed Image Text:3. Sucrose decomposes in aqueous solution into a mixture of two sugars, glucose and fructose. C„H„0, (aq) + H,0(1) I C,H,,0,(aq) + C,H,„O,(aq) The observed initial rates of decomposition of sucrose at two different initial sucrose concentrations at 25°C are: Rate ( M sec ') [Sucrose] 0.1 8.5 X 10 -3 1.71 X 102 0.2 Find the dependence of the reaction rate on the concentration of sucrose and compute the rate constant for the reaction.
Expert Solution
Step 1
  • Reaction rate means speed of the reaction under given conditions.
  • Reaction rate depends on concentration by Van't Hoff Differential method (as follows):-

         r1r2=(c1c2)n

          where,

          r1 and r2 are the reaction rates at two different concentration values (c1 and c2 ).

          and, 'n' is the order of the reaction.

  • One can find the order of the reaction(n) from this reaction rate dependence on concentration.
  • Rate constant(K) is the ratio of the reaction rate and the concentration of reactants raise to their order for the reaction.

         K=r[reactant]n

trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Reaction Rates
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS