Bond Average Bond Energies (per mole of bonds) H-H C-H C-C C=C 0-H C-O C=O 0=0 0-0 413 347 614 467 358 799* 495 146 Bond energy (kJ/mol) 432 The chemical equation for the combustion of ethanol is as follows: C₂H5OH +302 → 2CO₂ + 3H₂O Use the table of average bond energies above to calculate the total energy transferred in to break all these bonds in the reactants. You may find recreating the table below on scratch paper helpful in calculating the total energy transferred. Molecular Structure HH II H-C-C-O-H II нн Bond Broken C-H C-C C-O Bond Energy (kJ/mol) Number of Bonds Broken Net Energy (kJ/mol)
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.
What's the answer?
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
