3. The density of acetic anhydride is 1.08 g/mL. How many moles of acetic anhydride are used in this experiment

The moles of acetic acid used in the experiment has been 0.1058 mol.

Density has been defined as mass of a substance per unit volume. The density has been expressed as:

The moles have been the mass of the substance with respect to the molar mass. The moles of a substance has been given as:

The given sample of acetic acid has density = 1.08 g/ml

The volume of the sample used in the experiment has been 10 ml.

Substituting the values for the mass of acetic acid:

The mass of the acetic acid used has been 10.8 g.

The molar mass of acetic acid has been 102.09 g/mol.

Substituting the values for the moles of acetic acid:

The moles of acetic acid used in the experiment has been 0.1058 mol.

Learn more about density, here:

link

Number of moles = 0.1058 mol

Explanation:

Density = 1.08 g/mL

Volume = 10ml

Density = Mass / Volume

Mass = Density * Volume

Mass = 1.08 * 10 = 10.8g

The molar mass of acetic anhydride = 102.09 g/mol

Molar mass = Mass / Moles

Upon solving for moles;

Moles = Mass / Molar mass

Moles = 10.8 / 102.09 = 0.1058 mol