Investigation 5.5.1 ACTIVITY Calorimetry versus Enthalpies of Formation In this activity, you will use enthalpies of formation to determine the enthalpy change of a chemical reaction. Then, you will use the enthalpy values obtained from calorimetry experiments to calculate standard enthalpies of formation. Finally, you will compare the results of the two calculations. The calorimetry data is from an experiment involving a bomb calorimeter. During the experiment, the thermal energy released by the substance in the calorimeter is transferred directly to the calorimeter rather than to water. The quantity of energy transferred is determined using 9bomb = Cbomb X AT where Cbomb is the heat capacity of the calorimeter in J/°C. LS & SKILLS HANDBOOK Purpose To compare the experimental value of the enthalpy of combustion of ethanol with that derived from calculations based on enthalpies of formation for ethanol, water, and carbon dioxide. A2.4 Procedure 1. Determine the enthalpy of combustion per mole of ethanol using the experimental data in Table 1. Table 1 Data from Combustion of Ethanol in a Bomb Calorimeter Mass of ethanol 3.26 g Heat capacity of calorimeter 11.7 kJ/°C Initial temperature of calorimeter 21.5°C Final temperature of calorimeter 29.4 °C 2. Determine the enthalpy of combustion per mole of ethanol using the standard enthalpies of formation in Table 2. • Questioning • Researching • Hypothesizing • Predicting Table 2 Standard Enthalpies of Formation Substance • Planning • Controlling Variables • Performing ● • Observing H₂O(1) CO₂(g) C₂H5OH(1) SKILLS MENU • Analyzing • Evaluating • Communicating AH, (kJ/mol) -285.8 -393.5 -235.2 Analyze and Evaluate (a) Calculate the percent difference between the values you calculated in Steps 1 and 2. Explain any discrepancy between the two methods. KUTA Apply and Extend (b) Ethanol is commonly used as a fuel for cars and for heating homes. Based on your results, explain why ethanol makes a good fuel. KU (c) Calculate the enthalpy of combustion for ethanol using bond energies and compare it with the other values. K/U™A
Investigation 5.5.1 ACTIVITY Calorimetry versus Enthalpies of Formation In this activity, you will use enthalpies of formation to determine the enthalpy change of a chemical reaction. Then, you will use the enthalpy values obtained from calorimetry experiments to calculate standard enthalpies of formation. Finally, you will compare the results of the two calculations. The calorimetry data is from an experiment involving a bomb calorimeter. During the experiment, the thermal energy released by the substance in the calorimeter is transferred directly to the calorimeter rather than to water. The quantity of energy transferred is determined using 9bomb = Cbomb X AT where Cbomb is the heat capacity of the calorimeter in J/°C. LS & SKILLS HANDBOOK Purpose To compare the experimental value of the enthalpy of combustion of ethanol with that derived from calculations based on enthalpies of formation for ethanol, water, and carbon dioxide. A2.4 Procedure 1. Determine the enthalpy of combustion per mole of ethanol using the experimental data in Table 1. Table 1 Data from Combustion of Ethanol in a Bomb Calorimeter Mass of ethanol 3.26 g Heat capacity of calorimeter 11.7 kJ/°C Initial temperature of calorimeter 21.5°C Final temperature of calorimeter 29.4 °C 2. Determine the enthalpy of combustion per mole of ethanol using the standard enthalpies of formation in Table 2. • Questioning • Researching • Hypothesizing • Predicting Table 2 Standard Enthalpies of Formation Substance • Planning • Controlling Variables • Performing ● • Observing H₂O(1) CO₂(g) C₂H5OH(1) SKILLS MENU • Analyzing • Evaluating • Communicating AH, (kJ/mol) -285.8 -393.5 -235.2 Analyze and Evaluate (a) Calculate the percent difference between the values you calculated in Steps 1 and 2. Explain any discrepancy between the two methods. KUTA Apply and Extend (b) Ethanol is commonly used as a fuel for cars and for heating homes. Based on your results, explain why ethanol makes a good fuel. KU (c) Calculate the enthalpy of combustion for ethanol using bond energies and compare it with the other values. K/U™A
Chemistry for Engineering Students
3rd Edition
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.79PAE: A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50...
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Transcribed Image Text:Investigation 5.5.1 ACTIVITY
Calorimetry versus Enthalpies of
Formation
In this activity, you will use enthalpies of formation to
determine the enthalpy change of a chemical reaction.
Then, you will use the enthalpy values obtained from
calorimetry experiments to calculate standard enthalpies
of formation. Finally, you will compare the results of the
two calculations.
The calorimetry data is from an experiment involving
a bomb calorimeter. During the experiment, the thermal
energy released by the substance in the calorimeter is
transferred directly to the calorimeter rather than to water.
The quantity of energy transferred is determined using
abomb Cbomb X AT
where Cbomb is the heat capacity of the calorimeter in J/°C.
Å
Purpose
To compare the experimental value of the enthalpy of
combustion of ethanol with that derived from calculations
based on enthalpies of formation for ethanol, water, and
carbon dioxide.
SKILLS
HANDBOOK
A2.4
Procedure
1. Determine the enthalpy of combustion per mole of
ethanol using the experimental data in Table 1.
Table 1 Data from Combustion of Ethanol in a Bomb Calorimeter
Mass of ethanol
3.26 g
Heat capacity of calorimeter
11.7 kJ/°C
Initial temperature of calorimeter
21.5 °C
Final temperature of calorimeter
29.4 °C
2. Determine the enthalpy of combustion per mole of
ethanol using the standard enthalpies of formation in
Table 2.
• Questioning
• Researching
• Hypothesizing
• Predicting
Table 2 Standard Enthalpies of Formation
Substance
• Planning
• Controlling Variables
• Performing
• Observing
H₂O(1)
CO₂(g)
C₂H5OH(1)
SKILLS MENU
• Analyzing
• Evaluating
• Communicating
AH, (kJ/mol)
-285.8
-393.5
-235.2
Analyze and Evaluate
(a) Calculate the percent difference between the
values you calculated in Steps 1 and 2. Explain any
discrepancy between the two methods. K/U TA
Apply and Extend
(b) Ethanol is commonly used as a fuel for cars and for
heating homes. Based on your results, explain why
ethanol makes a good fuel. K/UA
(c) Calculate the enthalpy of combustion for ethanol
using bond energies and compare it with the other
values. K/UT/I
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