The thermite reaction,Fe2O3 + Al S Al2O3 + Feproduces so much heat that the Fe product melts. This reactionis used industrially to weld metal parts under water,where a torch cannot be employed. It is also a favorite chemicaldemonstration in the lecture hall (on a small scale).(a) Balance the chemical equation for the thermite reaction,and include the proper states of matter.(b) Calculate how many grams of aluminum are needed tocompletely react with 500.0 g of Fe2O3 in this reaction.(c) This reaction produces 852 kJ of heat per mole of Fe2O3reacted. How many grams of Fe2O3 are needed to produce1.00 * 104 kJ of heat?(d) If you performed the reverse reaction— aluminum oxideplus iron makes iron oxide plus aluminum—would thatreaction have heat as a reactant or a product?
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.
The thermite reaction,
Fe2O3 + Al S Al2O3 + Fe
produces so much heat that the Fe product melts. This reaction
is used industrially to weld metal parts under water,
where a torch cannot be employed. It is also a favorite chemical
demonstration in the lecture hall (on a small scale).
(a) Balance the chemical equation for the thermite reaction,
and include the proper
(b) Calculate how many grams of aluminum are needed to
completely react with 500.0 g of Fe2O3 in this reaction.
(c) This reaction produces 852 kJ of heat per mole of Fe2O3
reacted. How many grams of Fe2O3 are needed to produce
1.00 * 104 kJ of heat?
(d) If you performed the reverse reaction— aluminum oxide
plus iron makes iron oxide plus aluminum—would that
reaction have heat as a reactant or a product?
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