Aspirin (C9H8O4) is produced from salicylic acid (C7H6O3) and acetic anhydride (
ID: 885889 • Letter: A
Question
Aspirin (C9H8O4) is produced from salicylic acid (C7H6O3) and acetic anhydride (C4H6O3): C7H6O3 + C4H6O3 --> C9H8O4 + HC2H3O2. A- How much salicylic acid is required to produce 3.50x10^3 kg of aspirin, assuming that all of the salicylic acid is converted to aspirin? B- How much salicylic acid would be required if only 80% of the salicylic acid is converted to aspirin? C- What is the theoretical yeild of aspirin if 115 kg of salicylic acid is allowed to react with 75kg acetic anhydride? D- How much of the excess reactant is left over from the reaction in part C?
Explanation / Answer
molar mass of salicylic acid = 138 gm
molar mass of acetic anhydride = 102 gm
molar mass of aspirin = 180 gm
a)
mass of aspirin= 3.5*10^3 Kg = 3,500,000 gm
molar mass of aspirin = 180 gm
number of moles of aspirin = mass /molar mass
= 3,500,000 / 180
= 19444.44 mol
So number of moles of salicylic acid required= 19444.44 mol
molar mass of salicylic acid = 138 gm
mass of salicylic acid = moles * molar mass
= 19444.44 * 138
= 2,683,333 gm
= 2.68*10^3 Kg
b)
Let number of salicylic acid required be x mol
then 80 % of x = number of moles of aspirin
then 80 % of x = 19444.44 mol
x = 24305.55 mol
mass of salicylic acid = moles * molar mass
= 24305.55 * 138
= 3,354,166 gm
= 3.35*10^3 Kg
c)
number of moles of salicyclic acid = 115000 / 138 = 833.33 mol
number of moles of acetic anhydride= 75000 / 102 = 735 .3 mol
acetic anhydride is limiting reagent
number of moles of asprin produced = 735.3 mol
mass of aspirin = number of moles * molar mass
= 735.3* 180
= 132,353 gm
= 132.4 Kg
d)
735.3 mol of salicyclic acid will react
number of moles of salicylic acid left = 833.3 - 735.3 = 98 mol
mass of salicylic acid left = 98*138 = 13524 gm = 13.5 Kg
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