Determine the limiting reactant for the reaction? a)acetic anhydride b)salicylic
ID: 799667 • Letter: D
Question
Determine the limiting reactant for the reaction? a)acetic anhydride b)salicylic acid Determine the theoretical yield of aspirin for the reaction? Determine the percent yield of aspirin for the reaction? Determine the percent yield of aspirin for the reaction? Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2) . The balanced equation is (C4H6O3+C7H6O3--->C9H8O4+C2H4O2) In a laboratory synthesis, a student begins with 3.10mL of acetic anhydride (density=1.08g/ml) and 1.23g of salicylic acid. Once the reaction is complete, the student collects 1.20g of aspirin. Determine the limiting reactant for the reaction? a)acetic anhydride b)salicylic acid Determine the theoretical yield of aspirin for the reaction? Determine the percent yield of aspirin for the reaction?Explanation / Answer
3.00 mL of acetic anhydride @ 1.08 g/mL = 3.24 grams of acetic anhydride
use molar mass to find moles:
3.24 grams of C4H6O3 @ 102.09 g/mol = 0.031736 moles acetic anhydride
1.25 g of C7H6O3 @ 138.12 g/mol = 0.009050 moles salicylic acid
by the equation:
C4H6O3 + C7H6O3 --> C9H8O4 + C2H4O2
equal moles are required to react...
the answer to your first question is
the 0.009050 moles salicylic acid is your limiting reagent
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theoretical yield
by the equation:
C4H6O3 + C7H6O3 --> C9H8O4 + C2H4O2
0.009050 mol salicylic acid produces an equal number of moles of aspirin = 0.009050 mol aspirin
using molar mass:
0.009050 mol aspirin @ 180.16 g/mol C9H8O4 = 1.6305 grams of aspirin
your second answer
your theoretical yield , rounded to 3 sig figs is
1.63 grams of aspirin
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percent yield for the reaction
(1.22 g of aspirin / 1.63 grams of aspirin possible) times 100 = 74.83 %
your last answer, rounded to 3 sig figs is
74.8% yield
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