Homework Help is Here – Start Your Trial Now!
Science
Chemistry
5. The hydrolysis of ethyl ethanoate is a reversible reaction. The equation for the equilibrium is shown below. CH3COOC2H5 + H2O = CH3COOH + C2H5OH A student mixed together 8.0 mol ethyl ethanoate and 5.0 mol water. He also added a small amount of hydrochloric acid to catalyse the reaction. The student left the mixture until it had reached equilibrium at constant temperature. He found that 2.0 mol of ethanoic acid had formed. e. Write the expression for Kc for this equilibrium system. [1] Complete the table below to show the composition of the equilibrium mixture. [2] component CH3COOC2H5 H₂O CH3COOH C2H5OH initial amount/mol 8.0 5.0 0.0 0.0 equilibrium amount / mol 2.0 ii. Calculate Kc to an appropriate number of significant figures. State the units, if any. [3] b. The student left the mixture at a higher temperature until a new equilibrium had been reached. He again measured the equilibrium amount of ethanoic acid and found that it had increased. What conclusions can be drawn about the reaction and its equilibrium constant? [

5. The hydrolysis of ethyl ethanoate is a reversible reaction. The equation for the equilibrium is shown below. CH3COOC2H5 + H2O = CH3COOH + C2H5OH A student mixed together 8.0 mol ethyl ethanoate and 5.0 mol water. He also added a small amount of hydrochloric acid to catalyse the reaction. The student left the mixture until it had reached equilibrium at constant temperature. He found that 2.0 mol of ethanoic acid had formed. e. Write the expression for Kc for this equilibrium system. [1] Complete the table below to show the composition of the equilibrium mixture. [2] component CH3COOC2H5 H₂O CH3COOH C2H5OH initial amount/mol 8.0 5.0 0.0 0.0 equilibrium amount / mol 2.0 ii. Calculate Kc to an appropriate number of significant figures. State the units, if any. [3] b. The student left the mixture at a higher temperature until a new equilibrium had been reached. He again measured the equilibrium amount of ethanoic acid and found that it had increased. What conclusions can be drawn about the reaction and its equilibrium constant? [

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
None
5. The hydrolysis of ethyl ethanoate is a reversible reaction. The equation for the equilibrium is shown below. CH3COOC2H5 + H2O CH3COOH + C2H5OH A student mixed together 8.0 mol ethyl ethanoate and 5.0 mol water. He also added a small amount of hydrochloric acid to catalyse the reaction. The student left the mixture until it had reached equilibrium at constant temperature. He found that 2.0 mol of ethanoic acid had formed. e. Write the expression for Kc for this equilibrium system. [1] f. i. Complete the table below to show the composition of the equilibrium mixture. component initial amount / mol equilibrium amount / mol [2] CH3COOC2H5 8.0 H₂O CH3COOH C2H5OH 5.0 0.0 0.0 2.0 ii. Calculate Kc to an appropriate number of significant figures. State the units, if any. [3] b. The student left the mixture at a higher temperature until a new equilibrium had been reached. He again measured the equilibrium amount of ethanoic acid and found that it had increased. What conclusions can be drawn about the reaction and its equilibrium constant? [3]
Transcribed Image Text:5. The hydrolysis of ethyl ethanoate is a reversible reaction. The equation for the equilibrium is shown below. CH3COOC2H5 + H2O CH3COOH + C2H5OH A student mixed together 8.0 mol ethyl ethanoate and 5.0 mol water. He also added a small amount of hydrochloric acid to catalyse the reaction. The student left the mixture until it had reached equilibrium at constant temperature. He found that 2.0 mol of ethanoic acid had formed. e. Write the expression for Kc for this equilibrium system. [1] f. i. Complete the table below to show the composition of the equilibrium mixture. component initial amount / mol equilibrium amount / mol [2] CH3COOC2H5 8.0 H₂O CH3COOH C2H5OH 5.0 0.0 0.0 2.0 ii. Calculate Kc to an appropriate number of significant figures. State the units, if any. [3] b. The student left the mixture at a higher temperature until a new equilibrium had been reached. He again measured the equilibrium amount of ethanoic acid and found that it had increased. What conclusions can be drawn about the reaction and its equilibrium constant? [3]
Expert Solution
steps

Step by step

Solved in 4 steps with 7 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Theories of 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.
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