2 Al + Fe 2 O 3 → Al 2 O 3 + 2 Fe ∆H Fe 2 O 3 = -824.2 kJ/mol ∆H Al 2 O 3 = -1675.7 kJ/mol Fe203(s) + 2 Al(s) → 2 Fe(s) + A1203) The reaction of 5.00 g Fe203 (M.M - 160 g/mol) with excess Al(s) … The thermite reaction, in which powdered aluminum reacts with iron oxide, is highly exothermic. Aluminothermic reactions are exothermic chemical reactions using aluminium as the reducing agent at high temperature. asked Jun 29, 2017 in Chemistry by Diana. Fe 2 O 3 + 2 Al → 2 Fe + Al 2 O 3. uses aluminium powder and iron(III) oxide. If 0.79 moles of aluminum is consumed in the reaction, the heat released is equal to -851.5*0.79 = -672.685 kJ The process is industrially useful for production of alloys of iron. The thermite reaction. What mass of iron is formed when 725 kJ of heat are released? Fe2O3(s) + 2 Al(s) → 2 Fe(s) + Al2O3(s) The reaction of 5.00 g Fe2O3 with excess Al(s) evolves 26.6 kJ of energy in the form of heat. Fe 2 O 3 (s) + 2 Al(s) → 2 Fe(s) + Al 2 O 3 (s) The reaction of 5.00 g Fe 2 O 3 (M.M. Calculate the enthalpy change per mole of Fe2O3 reacted. The reaction of iron (III) oxide and aluminum can be represented by the equation: Fe 2 O 3 (s) + 2 Al (s) → Al 2 O 3 (s) + 2 Fe (s) This reaction is one of a class of reactions known as the “thermite” process, which has been used industrially for welding, the preparation of metals from their oxides, and the production of incendiary devices. Expressed in a chemical equation: reactants → products + energy The highly exothermic thermite reaction, in which aluminum reduces iron (III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. Answers: a) -5.32 kJ b) -1.33 ´ 102 kJ c) -2.12 ´ 104 kJ d) -2.12 ´ 102 kJ e) -8.50 ´ 102 kJ Exothermic Iron-Oxide and Aluminum Reaction. The most prominent example is the thermite reaction between iron oxides and aluminium to produce iron itself: . Fe2O3(s) + 2Al(s) ® 2Fe(s) + Al2O3(s) The reaction of 5.00 g Fe2O3 with excess Al evolves 26.6 kJ of energy in the form of heat. For every mole of aluminum that reacts with iron oxide, 851 kJ of heat is released. Calculate the enthalpy change per mole of Fe 2 O 3 reacted. Iron oxide reacts with aluminum in an exothermic reaction. It is the opposite of an endothermic reaction. When ignited, the mixture reacts vigorously because of the large difference in reactivity between aluminium and iron. a 47 g . Iron oxide reacts with aluminum in an exothermic reaction. = 160 g/mol) with excess Al(s) evolves 26.6 kJ of energy in the form of heat. Iron oxide reacts with aluminum in an exothermic reaction. The Iron that is produced by the reaction is melted because of the intense heat the thermite reaction produces. … 2Al(s) + Fe2O3(s) --> 2Fe(s) + Al2O3(s) ; DH = - 850 kJ. It is an exothermic reaction and results in its reactants, Aluminum Oxide and Iron, and heat of over 3000 degrees Celsius. 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