When sulfuric acid dissolves in water, a great deal if heat is given off. The enthalpy change for this process is called enthalpy of solution. To measure it, 175 g of water was placed in a coffee cup calorimeter and chilled to 10 degrees celsius. Then 49.0 g of pure sulfuric acid, also at 10 degrees celsius, was added, and the mixture was quickly stirred in the thermometer. The temperature rose rapidly to 14.9 degrees celsius. Assume the value of the specific heat of solution is 4.184j/g degree celsius. You may assume that the specific heat of the resulting sulfuric acid solution will also be 4.184j/g degrees celsius. Calculate q fr the formation of this solution and the enthalpy of solution in kilojoules per mole of H2SO4.
When sulfuric acid dissolves in water, a great deal if heat is given off. The enthalpy change for this process is called enthalpy of solution. To measure it, 175 g of water was placed in a coffee cup calorimeter and chilled to 10 degrees celsius. Then 49.0 g of pure sulfuric acid, also at 10 degrees celsius, was added, and the mixture was quickly stirred in the thermometer. The temperature rose rapidly to 14.9 degrees celsius. Assume the value of the specific heat of solution is 4.184j/g degree celsius. You may assume that the specific heat of the resulting sulfuric acid solution will also be 4.184j/g degrees celsius. Calculate q fr the formation of this solution and the enthalpy of solution in kilojoules per mole of H2SO4.
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
When sulfuric acid dissolves in water, a great deal if heat is given off. The enthalpy change for
this process is called enthalpy of solution. To measure it, 175 g of water was placed in a coffee cup calorimeter and chilled to 10 degrees celsius. Then 49.0 g of pure sulfuric acid, also at 10 degrees celsius, was added, and the mixture was quickly stirred in the thermometer. The temperature rose rapidly to 14.9 degrees celsius. Assume the value of the specific heat of solution is 4.184j/g degree celsius. You may assume that the specific heat of the resulting sulfuric acid solution will also be 4.184j/g degrees celsius. Calculate q fr the formation of this solution and the enthalpy of solution in kilojoules per mole of H2SO4.
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
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