Question 30 of 37 Calculate the enthalpy of combustion (kJ/mol) of ethyl stearate (C20H4002), an important component of many biodiesel fuels made from soybean oil and ethanol, given the following standard enthalpies of formation: CO2(g) = -393.5 kJ/mol H2O(1) = -285.8 kJ/mol C20H40O2(1) = -984.6 kJ/mol
Question 30 of 37 Calculate the enthalpy of combustion (kJ/mol) of ethyl stearate (C20H4002), an important component of many biodiesel fuels made from soybean oil and ethanol, given the following standard enthalpies of formation: CO2(g) = -393.5 kJ/mol H2O(1) = -285.8 kJ/mol C20H40O2(1) = -984.6 kJ/mol
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
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Calculate the enthalpy of combustion (kJ/mol) of ethyl stearate
(C20H4002), an important component of many biodiesel fuels made
from soybean oil and ethanol, given the following standard enthalpies
of formation:
CO2(g) = -393.5 kJ/mol
-11689.4 kJ/mol
H2O(I) = -285.8 kJ/mol
C20H40O2(1) = -984.6 kJ/mol
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