Homework Help is Here – Start Your Trial Now!
Science
Chemistry
I need help with 6 through 10, and I think it's all supposed to be in three sig figs. Can you help me with this?

I need help with 6 through 10, and I think it's all supposed to be in three sig figs. Can you help me with this?

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

I need help with 6 through 10, and I think it's all supposed to be in three sig figs. Can you help me with this?

3-6: Heat of Combustion: Sugar The heat of combustion (AHcomb) is the heat of reaction for the complete burning (reacting with O2) of one mole of a substance to form CO, and H,O. Calorimetry experiments that measure the heat of combustion can be performed at constant volume using a device called a bomb calorimeter. In a bomb calorimeter a sample is burned in a constant-volume chamber in the presence of oxygen at high pressure. The heat that is released warms the water surrounding the chamber. By measuring the temperature increase of the water, it is possible to calculate the quantity of heat released during the combustion reaction. In this assignment you will calculate the heat of combustion of sugar (sucrose, C12H22O11). The calorimeter has already been calibrated by combusting benzoic acid. 1. Start Virtual ChemLab, select Thermodynamics, and then select Heat of Combustion: Sugar from the list of assignments. The lab will open in the Calorimetry laboratory with the bomb calorimeter out and disassembled and with a sample of sugar in the calorimeter cup on the balance. The balance has already been tared. 2. Record the mass of the sugar sample from the balance. If you cannot read it, click on the Balance area to zoom in, record the mass in the data table below and return to the laboratory. 3. Double-click the following (in numerical order) to assemble the calorimeter: (1) the cup on the balance pan, (2) the bomb head, (3) the screw cap, and (4) the bomb. Click the calorimeter lid to close it. Combustion experiments can take a considerable length of time. Click the clock on the wall labeled Accelerate to accelerate the laboratory time. 4. Click the bomb control panel and the plot window to bring them to the front. Click on the Save button to save data to the lab book. Allow the graph to proceed for 20-30 seconds to establish a baseline temperature. 5. Click Ignite and observe the graph. When the temperature has leveled off (up to 5 minutes of laboratory time), click Stop. A data link icon will appear in the lab book. Click the data link icon to view the collected data. Record the temperature before and after ignition of the sugar sample in the data table. Data Table sucrose (C12H2½O11) 0.9715g mass of sample (g) initial temperature (°C) 24.996 final temperature (°C) 26.518 6. Write a complete balanced chemical equation for the combustion of sucrose. 7. Calculate AT for the water using AT = |T;- T|.
Transcribed Image Text:3-6: Heat of Combustion: Sugar The heat of combustion (AHcomb) is the heat of reaction for the complete burning (reacting with O2) of one mole of a substance to form CO, and H,O. Calorimetry experiments that measure the heat of combustion can be performed at constant volume using a device called a bomb calorimeter. In a bomb calorimeter a sample is burned in a constant-volume chamber in the presence of oxygen at high pressure. The heat that is released warms the water surrounding the chamber. By measuring the temperature increase of the water, it is possible to calculate the quantity of heat released during the combustion reaction. In this assignment you will calculate the heat of combustion of sugar (sucrose, C12H22O11). The calorimeter has already been calibrated by combusting benzoic acid. 1. Start Virtual ChemLab, select Thermodynamics, and then select Heat of Combustion: Sugar from the list of assignments. The lab will open in the Calorimetry laboratory with the bomb calorimeter out and disassembled and with a sample of sugar in the calorimeter cup on the balance. The balance has already been tared. 2. Record the mass of the sugar sample from the balance. If you cannot read it, click on the Balance area to zoom in, record the mass in the data table below and return to the laboratory. 3. Double-click the following (in numerical order) to assemble the calorimeter: (1) the cup on the balance pan, (2) the bomb head, (3) the screw cap, and (4) the bomb. Click the calorimeter lid to close it. Combustion experiments can take a considerable length of time. Click the clock on the wall labeled Accelerate to accelerate the laboratory time. 4. Click the bomb control panel and the plot window to bring them to the front. Click on the Save button to save data to the lab book. Allow the graph to proceed for 20-30 seconds to establish a baseline temperature. 5. Click Ignite and observe the graph. When the temperature has leveled off (up to 5 minutes of laboratory time), click Stop. A data link icon will appear in the lab book. Click the data link icon to view the collected data. Record the temperature before and after ignition of the sugar sample in the data table. Data Table sucrose (C12H2½O11) 0.9715g mass of sample (g) initial temperature (°C) 24.996 final temperature (°C) 26.518 6. Write a complete balanced chemical equation for the combustion of sucrose. 7. Calculate AT for the water using AT = |T;- T|.
8. Calculate the moles of sucrose in the sample (MWguerose = 342.3 g/mol). 9. AHcomb for sucrose can be calculated using AH0omb = (C,ystem AT)/n , where n is the moles of sucrose in ´system the sample and Csystem is the heat capacity of the calorimetric system. Use 10.310 kJ/K for Cystem and calculate the heat of combustion, in kJ/mol, for sucrose. 10. If the accepted value for the heat of combustion for sugar is 5639 kJ/mol calculate the percent error. |your answer – accepted answer| -× 100 % Error accepted answer % Error = This experiment does not consider that all of the conditions are standard state conditions; therefore, you are calculating AHcomb not AH°comb.
Transcribed Image Text:8. Calculate the moles of sucrose in the sample (MWguerose = 342.3 g/mol). 9. AHcomb for sucrose can be calculated using AH0omb = (C,ystem AT)/n , where n is the moles of sucrose in ´system the sample and Csystem is the heat capacity of the calorimetric system. Use 10.310 kJ/K for Cystem and calculate the heat of combustion, in kJ/mol, for sucrose. 10. If the accepted value for the heat of combustion for sugar is 5639 kJ/mol calculate the percent error. |your answer – accepted answer| -× 100 % Error accepted answer % Error = This experiment does not consider that all of the conditions are standard state conditions; therefore, you are calculating AHcomb not AH°comb.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Tools in Analytical Chemistry
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