Question

aspirin C6H4(CO2)(CO2CH3),can be prepared in the chemistry laboratory by the reactions of salicylic acid, C6H4(CO2H)(OH),with acetic anhydride(CH3CO)2O.what volume of acetic anhydride(density,1.0820g/cm3) is required to produce 1.00kg of aspirin, assuming a 100% yield

Answer 1

To calculate the volume of acetic anhydride needed to produce 1.00kg of aspirin, you need to find the molar mass of acetic anhydride, convert the mass of aspirin to moles, and use the density of acetic anhydride to convert the volume from grams to milliliters.

Step-by-step explanation:

To calculate the volume of acetic anhydride needed to produce 1.00kg of aspirin, we need to start by finding the molar mass of acetic anhydride, which is 102.09 g/mol. Next, we can convert the mass of aspirin to moles by dividing it by its molar mass, which is 180.16 g/mol. Since the reaction is 1:1 between acetic anhydride and aspirin, we can assume that we need an equal number of moles of acetic anhydride. Finally, we can use the density of acetic anhydride to convert the volume from grams to milliliters. The calculation would be:

Mass of acetic anhydride = moles of aspirin x molar mass of acetic anhydride = 1.00 kg / (180.16 g/mol) x (102.09 g/mol)

Volume of acetic anhydride in mL = mass of acetic anhydride / density of acetic anhydride = (mass of acetic anhydride in g) / (density of acetic anhydride in g/mL)

By plugging in the values, we can calculate the volume of acetic anhydride required to produce 1.00kg of aspirin.

Answer 2

262mol 1=kg
g=1000
from stoichoimetry

x=102*1000/360
x=102000/360
x=283.33

density =m/v
=283.33/1.082
=262mol