The experimental enthalpy of decomposition of H2O2 was determined using another coffee-cup calorimetry. A sample of H2O2 solution was placed in the calorimeter and the initial temperature of H2O2 solution and the calorimeter was measured. Then, KI solution was added to the solution to catalyze the decomposition of H2O2 to H2O. This resulted to an increase of 16.5ºC in the temperature. Determine the experimental enthalpy of decomposition per mole of H2O2 given the following additional information. Express your answer in kJ/mol and in 2 decimal places.
The experimental enthalpy of decomposition of H2O2 was determined using another coffee-cup calorimetry. A sample of H2O2 solution was placed in the calorimeter and the initial temperature of H2O2 solution and the calorimeter was measured. Then, KI solution was added to the solution to catalyze the decomposition of H2O2 to H2O. This resulted to an increase of 16.5ºC in the temperature. Determine the experimental enthalpy of decomposition per mole of H2O2 given the following additional information. Express your answer in kJ/mol and in 2 decimal places.
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...
Related questions
Question
The experimental enthalpy of decomposition of H2O2 was determined using another coffee-cup calorimetry. A sample of H2O2 solution was placed in the calorimeter and the initial temperature of H2O2 solution and the calorimeter was measured. Then, KI solution was added to the solution to catalyze the decomposition of H2O2 to H2O. This resulted to an increase of 16.5ºC in the temperature. Determine the experimental enthalpy of decomposition per mole of H2O2 given the following additional information. Express your answer in kJ/mol and in 2 decimal places.
moles H2O2: 0.018 mol
Ccal: 53.82 J/oC
mass of the solution (mainly water): 35.2 g
Cp of water: 4.184 J/goC
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY