In this virtual lab, calorimetry will be performed to determine the heat 100 capacity, Ceal , of a coffee cup calorimeter. Imagine that, in lab the mass of a piece of iron, mpe, is recorded as mfe = 51.56 g In the next step of the lab (as shown in the image) the piece of metal is heated up. Record the metal's highest temperature, Tre- (Read to the tenths place) Tre = °C Next, the metal is dropped into the coffee cup calorimeter. Please continue to the next image. In another step of this lab, the mass of ethanol (methanol ) in a coffee cup is recorded as methanol = 63.87 g The initial temperature of the ethanol, Tethanol.1 » is given to be 14.00 °C. In the next step of the lab (as shown in the image) the hot piece of iron is placed into the cool ethanol. Record the final temperature of the ethanol. Note this also serves as the final temperature of the metal. In the final step, using the specific heats (2.420 and 0.4498 J/(g · °C) for ethanol and iron, respectively) and the mass of ethanol and iron given, calculate the heat, taken up by the ethanol, qethanol , and the heat given off by the metal, qiron , and record them. Tethanol,2 °C Gethanol = J 9Fe = J Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a qethanol Value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter. 9cal = J The observed final temperature of iron from this trial was 94.64 °C, whereas the initial and final temperatures of ethanol were 14.50 °C and 24.00 °C, respectively. Using this information, calculate the heat capacity, Ccal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?
In this virtual lab, calorimetry will be performed to determine the heat 100 capacity, Ceal , of a coffee cup calorimeter. Imagine that, in lab the mass of a piece of iron, mpe, is recorded as mfe = 51.56 g In the next step of the lab (as shown in the image) the piece of metal is heated up. Record the metal's highest temperature, Tre- (Read to the tenths place) Tre = °C Next, the metal is dropped into the coffee cup calorimeter. Please continue to the next image. In another step of this lab, the mass of ethanol (methanol ) in a coffee cup is recorded as methanol = 63.87 g The initial temperature of the ethanol, Tethanol.1 » is given to be 14.00 °C. In the next step of the lab (as shown in the image) the hot piece of iron is placed into the cool ethanol. Record the final temperature of the ethanol. Note this also serves as the final temperature of the metal. In the final step, using the specific heats (2.420 and 0.4498 J/(g · °C) for ethanol and iron, respectively) and the mass of ethanol and iron given, calculate the heat, taken up by the ethanol, qethanol , and the heat given off by the metal, qiron , and record them. Tethanol,2 °C Gethanol = J 9Fe = J Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a qethanol Value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter. 9cal = J The observed final temperature of iron from this trial was 94.64 °C, whereas the initial and final temperatures of ethanol were 14.50 °C and 24.00 °C, respectively. Using this information, calculate the heat capacity, Ccal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?
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
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 4 steps
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