Diamond Carbide
September 28th, 2009
percent yield?
The abrasive carborundum (silicon carbide) is one of the hardest materials known, second only to diamond (pure carbon). It can be produced by heating a mixture of sand (silicon dioxide) and coke (distilled coal that is almost pure amorphous carbon) in a furnace:
SiO2(l) + 3C(s) → SiC(s) + 2CO(g)
Calculate the theoretical yield of carborundum when 32.3 g of sand are heated with 25.5 g of coke.
Calculate the number of moles of reactants that will remain in the furnace if the reaction goes to completion.
Sand: ; Coke:
Calculate the percent yield of carborundum if only 19.0 g were actually obtained in the above process. Enter your answer without the % sign.
Moles SiO2 = 32.3 / 60.0855 g/mol =0.538
Moles C = 25.5 g / 12.011 = 2.12
SiO2 is the limiting reactant
Moles SiC = 0.538 => 0.538 mol x 40.0965 g/mol =21.6 g
% = 19.0 x 100 / 21.6 = 88.0
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