Question Solved1 Answer The thermite reaction involves aluminum and iron(III) oxide,2Al(s) + Fe2O3(s) ( Al2O3(s) + 2Fe(l)This reaction is highly exothermic and the liquid iron formed is used to weld metals. Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. (The ΔH°f for Fe(l) is 12.40 kJ/mol; ΔH°f for Fe2O3(s) is -822.2 kJ/mol; ΔH°f for Al2O3(s) is -1669.8kJ/mol)

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The thermite reaction involves aluminum and iron(III) oxide,
2Al(s) + Fe2O3(s) ( Al2O3(s) + 2Fe(l)

This reaction is highly exothermic and the liquid iron formed is used to weld metals. Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. 

(The ΔH°f for Fe(l) is 12.40 kJ/mol; ΔH°f for Fe2O3(s) is -822.2 kJ/mol;
ΔH°f for Al2O3(s) is -1669.8kJ/mol)

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Step 1The enthalpy change of a chemical reaction can be calculated by the standard heat of formation of the reactants and the products. The standard enthalpy change of the reaction is given by:DeltaH_("reaction ")^(o)=sumH_(f(" product "))^(o)-sumH_(("reactant "))^(o)The given chemical reaction is as follows:2Al(s) + Fe2O3(s) ( Al2O3(s) + 2Fe(l)The heat of formation of the reactants and the products is as follows:ΔHf° for Fe(l) is =12.40 kJ/molΔHf° for Fe2O3(s) is = -822.2 kJ/molΔHf° for Al2O3(s) is -1669.8kJ/molΔHf° for Al(s) = 0 (according to the definition)Step 2Calculation of molar enthalpy change of the reaction:DeltaH_("reaction ")^(o)=sum(-1669.8)+(12.10 ... See the full answer