Can someone explain in detail the steps to do thisproblem? The reaction between

Question

Can someone explain in detail the steps to do thisproblem? The reaction between aluminum and iron (III) oxide cangenerate temperatures approaching 3000 degrees Celsius and is usedin welding metals: In one process, 124 g of Al are reacted with 601 g ofFe2O3. (a) Calculate the mass (in grams) ofAl2O3 formed. (b) How much of the excess reagent is left at the end of thereaction?

Explanation / Answer

Molar mass of Al - 27 gms/mol. => No. of moles = mass/molar mass = 124/27 = 4.59 moles Molar mass of Fe2O3 = 160 gm/mol => No. of moles = 601/160 moles = 3.76 moles Now, 2 moles Al reacts with - 1mol Fe2O3 => 4.59 moles Al reacts with - 2.29 molesFe2O3 a) No. of moles of Al2O3 formed = no. ofmoles of Fe2O3 consumed = 2.29 moles Mass of Al2O3 formed = 2.29 x 102 gms/mol =233.6 gms b) No. of moles of Fe2O3 remaining =3.76-2.29 = 1.47 moles Mass of Fe2O3 remaining = 1.47 x 160 gms =235.2 gms

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