Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Figure 2: Example Graph Temperature vs. Time: Cold Water + Hot Water T= 48.4 °C at time of mixing T = 35.7 °C at time of mixing T. = 23.8 °C at time of mixing 6 7 8 9. 10 11 12 13 1 2 3 4 5 Time (min) Tem perature("C)

Figure 2: Example Graph Temperature vs. Time: Cold Water + Hot Water T= 48.4 °C at time of mixing T = 35.7 °C at time of mixing T. = 23.8 °C at time of mixing 6 7 8 9. 10 11 12 13 1 2 3 4 5 Time (min) Tem perature("C)

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

Calculate the heat capacity of the calorimeter for which the sample data in Figure 2 was collected. Assume that mh=mc=50.0g.

2-3 Figure 2: Example Graph Temperature vs. Time: Cold Water + Hot Water Th = 48.4 °C at time of mixing T = 35.7 °C at time of mixing' T. = 23.8 °C at time of mixing 1. 2 3 4 6 7 8. 10 11 12 13 Time (min) Once the heat capacity of the calorimeter is known, AH may be calculated for reactions 1, 2 and 3 by measuring their temperature increases upon reaction. Since the reactions are done at constant pressure, the heat released by the reaction, q,, is equal to the enthalpy change for that reaction: 9r = CAT heat released by the system (reaction) = heat absorbed by the surroundings (solution + calorimeter) = Asoln + 9cal = msoln Csoln AT + Ccal AT or 9r = -(msoln Csoln + Ccal)AT AT for these reactions is obtained from graphs by extrapolating Tf and T¡ to the time of mixing. The graphs will be similar to Figure 2 except that reactions 2 and 3 will have only two lines (two temperatures) rather than three. AH, will be determined for each of reactions 1, 2, and 3. AH3 will also be calculated using Hess's Law as described on the first page of this experiment. Comparison of the experimental and Hess's Law values of AH3 will provide a test for Hess's Law. Tem perature ("C)
Transcribed Image Text:2-3 Figure 2: Example Graph Temperature vs. Time: Cold Water + Hot Water Th = 48.4 °C at time of mixing T = 35.7 °C at time of mixing' T. = 23.8 °C at time of mixing 1. 2 3 4 6 7 8. 10 11 12 13 Time (min) Once the heat capacity of the calorimeter is known, AH may be calculated for reactions 1, 2 and 3 by measuring their temperature increases upon reaction. Since the reactions are done at constant pressure, the heat released by the reaction, q,, is equal to the enthalpy change for that reaction: 9r = CAT heat released by the system (reaction) = heat absorbed by the surroundings (solution + calorimeter) = Asoln + 9cal = msoln Csoln AT + Ccal AT or 9r = -(msoln Csoln + Ccal)AT AT for these reactions is obtained from graphs by extrapolating Tf and T¡ to the time of mixing. The graphs will be similar to Figure 2 except that reactions 2 and 3 will have only two lines (two temperatures) rather than three. AH, will be determined for each of reactions 1, 2, and 3. AH3 will also be calculated using Hess's Law as described on the first page of this experiment. Comparison of the experimental and Hess's Law values of AH3 will provide a test for Hess's Law. Tem perature ("C)
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Measurement
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