Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol).
C7H6O3(s) + C4H6O3(λ) → C9H8O4(s) + C2H4O2(λ)
If you mix 5.00 grams of each reactant, how many grams of aspirin (M = 180.2 g/mol) can theoretically by obtained?
a.2.83 g
b.3.83 g
c.6.52 g
d.10.0 g
e.8.82 g
2007-05-30 05:05:25 · 4 answers · asked by kallystarr 1 in Science & Mathematics ➔ Chemistry
5 grams salicylic acid = 5g * mole/138.1g = 0.0362 moles
5 grams acetic anhydride = 5g * mole/102.1g = 0.04897 moles
Salicylic acid is limiting reagent
so you would expect 0.0362 moles product
0.0362 moles * 180.2 g/moles = 6.52 g
2007-05-30 05:19:18 · answer #1 · answered by Dr Dave P 7 · 0⤊ 0⤋
c.
Salicylic acid has the greater molecular weight of the two reagents, and thus (since stoichiometry is 1:1 for this reaction), is your limiting reagent in this problem.
5 g / (138.1 g / mol) = 0.0362 mol
With 1:1 stoichiometry, you'll make 0.0362 mol of aspirin with 0.0362 mol of each reagent.
0.0362 mol * 180.2 g/mol = 6.52 g aspirin
2007-05-30 05:13:43 · answer #2 · answered by not gh3y 3 · 0⤊ 0⤋
5.00 / 138.1 = 0.0362 moles acid
5.00 / 102.1 = 0.0490 moles acetic anhydride
the ratio between reactants is 1 : 1 so salycilic acid is the limiting reactant
we get 0.0362 mole of aspirin
0.0362 x 180.2 = 6.52 g
the answer is c
2007-05-30 05:18:15 · answer #3 · answered by Non più attiva su answers 7 · 0⤊ 0⤋
c.6.52 g
2007-05-30 05:30:53 · answer #4 · answered by ag_iitkgp 7 · 0⤊ 0⤋