Aspirin can be synthesized in the lab by combining salicylic acid ( C7H6O3) and acetic anhydride ( C4H6O3) to form aspirin (C9H8O4) and acetic acid ( C2H4O2). The balanced equation for this reaction is
C7H6O3+C4H6O3⟶C9H8O4+C2H4O2
A student started with 5.30 mL acetic anhydride (density=1.08 g/mL) and 1.01 g salicylic acid. The student synthesized 1.25 g of aspirin.
What is the limiting reactant?
Also calculate the yield the theoretical and percentage yield of aspirin ( C9H8O4). If somebody could please explain this, I'd appreciate it. Thank you.
Aspirin chemistry equation?
2020-06-14 8:05 pm
回答 (2)
2020-06-14 11:52 pm
✔ 最佳答案
Molar mass of C₇H₆O₃ (salicylic acid) = (12×7 + 1×6 + 16×3) g/mol = 138 g/molMolar mass of C₄H₆O₃ (acetic anhydride) = (12×4 + 1×6 + 16×3) g/mol = 102 g/mol
Molar mass of C₉H₈O₄ (aspirin) = (12×9 + 1×8 + 16×4) g/mol = 180 g/mol
Initial moles of salicylic acid = (1.01 g) / (138 g/mol) = 0.007319 mol
Initial moles of acetic anhydride = (5.30 × 1.08 g) / (102 g/mol) = 0.05612 mol
salicylic acid + acetic anhydride → aspirin + acetic acid
Mole ratio (salicylic acid) : (acetic anhydride) = 1 : 1
As (Moles of acetic anhydride) > (Moles of salicylic acid),
salicylic acid is the limiting reactant.
According to the equation, mole ratio (salicylic acid) : (aspirin) = 1 : 1
Maximum moles of aspirin produced = 0.007319 mol
Theoretical yield of aspirin = (0.007319 mol) × (180 g/mol) = 1.32 g
Percentage yield of aspirin = (1.25/1.32) × 100% = 94.7%
2020-06-14 9:15 pm
Convert the starting amounts of the two reagents to moles.
The reaction uses equal moles of both, so whichever there was less of is the limiting reagent.
The theoretical yield is the amount of aspirin that would be produced if all of the limiting reagent reacted.
Percentage yield is (actual yield)/(theoretical yield)
The reaction uses equal moles of both, so whichever there was less of is the limiting reagent.
The theoretical yield is the amount of aspirin that would be produced if all of the limiting reagent reacted.
Percentage yield is (actual yield)/(theoretical yield)
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