Percent Yield?
- any help will be appreciated –
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 35.5 g of sand are heated with 16.4 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 14.9 g were actually obtained in the above process. Enter your answer without the % sign.
Number of moles of SiO2 used = 35.5g/(60.09gmol-1)
= 0.5908 mol
Number of moles of C used = 16.4g/(12gmol-1)
= 1.3667 mol
from the reaction equation, 1 moles of sand reacts completely with 3 moles of coke. Hence, 1.7724 mol of coke is needed to reacts completely with 0.5908 mol of sand. The limiting reagent of this reaction is coke.
3 mol of coke yields 1 mol of carborundum
Theoretical yield of SiC = 1/3 (1.3667mol) x (40.09gmol-1)
= 18.2637g
The number of mole of sand reacted = 1/3 (1.3667mol)
= 0.4556 mol
The number of mole of sand remain in the furnace
= 0.5908mol – 0.4556mol = 0.1352mol
Percentage yield = (14.9g/18.2637g) x 100
= 81.58
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