The thermite reaction, Fe2O3 + Al → Al2O3 + Fe produces so much heat that the Fe product melts. 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 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. This amount of energy change associated with a chemical reaction can be included in the chemical equation in this format: Fe2O3 + Al → Al2O3 + Fe (still unbalanced) ΔH = – 852 kJ where ΔH refers to the enthalpy change, the negative sign indicates that energy is produced by the chemical reaction, and the indicated quantity of energy is stoichiometrically equivalent to the number of moles indicated by the coefficients of the balanced equation. In this case, 1 mol Fe2O3 = 852 kJ = x mol Al = y mol Al2O3 = z mol Fe, where x, y and z are the coefficients in the balanced equation (which you need to work out in item 2.a) This shorthand way of describing a chemical reaction that shows the associated energy change is called a thermochemical equation. How many grams of Fe2O3 are needed to produce 1.00 x 104 kJ of heat?
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 → Al2O3 + Fe produces so much heat that the Fe product melts.
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. This amount of energy change associated with a
Fe2O3 + Al → Al2O3 + Fe (still unbalanced) ΔH = – 852 kJ
where ΔH refers to the enthalpy change, the negative sign indicates that energy is produced by the chemical reaction, and the indicated quantity of energy is stoichiometrically equivalent to the number of moles indicated by the coefficients of the balanced equation. In this case,
1 mol Fe2O3 = 852 kJ = x mol Al = y mol Al2O3 = z mol Fe,
where x, y and z are the coefficients in the balanced equation (which you need to work out in item 2.a)
This shorthand way of describing a chemical reaction that shows the associated energy change is called a thermochemical equation.
How many grams of Fe2O3 are needed to produce 1.00 x 104 kJ of heat?
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