Simple Stoichiometry Problem

3.0 grams of salicylic acid C7H8O3 reacts with 6 mL of acetic anhydride C4H6O3 (1.08g/ml) to make acetylsalicylic acid C9H10O4 and ethanoic acid C2H4O2. How much acetysalicylic acid was made?
Show all work, including which reactant was limiting, the mass of acetic anhydride,etc,etc.
Thanks!!

first you want to write a balanced equation for the reaction (this is an easy one to balance)

C7H8O3 + C4H6O3 ---> C9H10O4 + C2H4O2

this is a limiting reagent problem so you have to take both the masses it gives you for the reactants and calculate how much C9H10O4 could possibly be made

start with the salicylic acid and use stoichiometry to get to the grams of acetylsalicylic acid

3.0 g C7H8O3 x (1 mol C7H8O3/ 140 g C7H8O3) x (1 mol C9H10O4/1 mol C7H8O3) x (182 g C9H10O4/ 1 mol C9H10O4)

= 3.9 g acetylsalicylic acid

now do the same process starting with the acetic anhydride

6 mL C4H6O3 x (1.08 g C4H6O3/ 1 mL C4H6O3) x (1 mol C4H6O3/ 102 g C4H6O3) x (1 mol C9H10O4/ 1 mol C4H6O3) x (182 g C9H10O4/ 1 mol C9H10O4)

=11.6 g acetylsalicylic acid

now to determine the limiting reagent, you have to pick the reactant that can make the least amount of the product. this is because once this reactant is used up, the reaction must stop because there is nothing left to react with. therefore, it limits the reaction (limiting reagent)

so the limiting reagent here is salicylic acid
and the mass of acetic acetysalicylic acid would be 3.9 grams

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