5. Use the data in the following tables and answer the following questions. a) The experimental data (table 1.) is from the combustion of ethanol in a bomb calorimeter. Use the data to determine the enthalpy of combustion per mole of ethanol. The quantity of energy transferred to the calorimeter can be solved using the equation Qbomb = Chomb* AT b)Use the standard enthalpies of formation (Table 2) to determine the enthalpy of combustion per mole of ethanol. c) Explain any discrepancies (2 reasons) between the values calculated in questions a. and b. 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 Table 2 Standard Enthalpies of Formation Substance H₂O( CO₂(g) C₂H₂OH() AH, (kJ/mol) -285.8 -393.5 -235.2
5. Use the data in the following tables and answer the following questions. a) The experimental data (table 1.) is from the combustion of ethanol in a bomb calorimeter. Use the data to determine the enthalpy of combustion per mole of ethanol. The quantity of energy transferred to the calorimeter can be solved using the equation Qbomb = Chomb* AT b)Use the standard enthalpies of formation (Table 2) to determine the enthalpy of combustion per mole of ethanol. c) Explain any discrepancies (2 reasons) between the values calculated in questions a. and b. 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 Table 2 Standard Enthalpies of Formation Substance H₂O( CO₂(g) C₂H₂OH() AH, (kJ/mol) -285.8 -393.5 -235.2
Chemistry by OpenStax (2015-05-04)
1st Edition
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 80E: Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil. (a) Write the...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:5. Use the data in the following tables and answer the following questions.
a) The experimental data (table 1.) is from the combustion of ethanol in a bomb calorimeter. Use the data to
determine the enthalpy of combustion per mole of ethanol.
The quantity of energy transferred to the calorimeter can be solved using the equation
Qbomb = Chomb* AT
b)Use the standard enthalpies of formation (Table 2) to determine the enthalpy of combustion per mole of
ethanol.
c) Explain any discrepancies (2 reasons) between the values calculated in questions a. and b.
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
Table 2 Standard Enthalpies of Formation
Substance
H₂O(l)
CO₂(g)
C₂H₂OH()
AH,* (kJ/mol)
-285.8
-393.5
-235.2
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