A student begins with 2.22 g of salicylic acid (Mole weight =138 g/mol) and 4.04

Question

A student begins with 2.22 g of salicylic acid (Mole weight =138 g/mol) and 4.04 mL of acetic anhydride ( mole weight= 102 g/mol, density= 1.081 g/mol) in the preparation of aspirin. Show all calculations Please!!! I really need to know the proces of how you got the answer i have a big test on this tommorrow and could really use someones help. It would really help if you showed all calculations and all steps.   

A. How many moles of salicylic acid were used
B How many moles of acetic anhydride were used?
C. Which compound is the limiting reagant in the preparation of aspirin?
D Calculate the theoretical yield for the reaction in moles and in grams of aspirin

Can you also please help me define and explain what theese mean...

1. Analgesic

2. Antipyretic

Explanation / Answer

Chemical Reaction: (already balanced)

salicylic acid (C7H6O3) + acetic anhydride (C4H6O3) ===> aspirin (C9H8O4) + acetic acid (C2H4O2)
______________________________________...

actual mol sal.acid = 2.22 g / 138 g/mol = 0.0161 mol
actual mol of acet.anhy. = [(4.04 mL)(1.081 g/mL)] / 102 g/mol = 0.0428 mol

Determine the limiting reactant. I assume, you know how to find it so I'm not going to explain it further.

theoretical mol of sal. acid that will react with acet. anhy = 0.0428 mol x (1 mol sal.acid / 1 mol acet.anhy.) = 0.0428 mol


Limiting reactant is salicylic acid:
______________________________

To calculate for the theoretical yield of aspirin, use the actual amount of the limiting reactant for stoichiometric analysis.

theoretical yield (in moles) = 0.0161 mol x (1 mol aspirin / 1 mol sal. acid)
theoretical yield (in moles) = 0.0161 mol of aspirin (answer)
______________________________________...

Theoretical yield (in grams) = 0.0161 mol x molar mass of aspirin
theoretical yield (in grams) = __________ (answer)

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