given the density of acetic anhydride to be 1.05 g/mL, what was the mass of the acetic anhydride added to the reaction? How many moles of acetic acid were added?
To find the mass of acetic anhydride added to the reaction, we need to know the volume of the acetic anhydride added. Without that information, we cannot calculate the exact mass.
However, we can calculate the number of moles of acetic acid added if we know the volume of acetic anhydride and assume it completely converts to acetic acid.
Let's say the volume of acetic anhydride added to the reaction is V mL.
To calculate the number of moles of acetic acid, we will use the formula:
moles = mass / molar mass.
The molar mass of acetic acid (CH3COOH) is:
(12.01 g/mol x 2) + (1.01 g/mol x 4) + (16.00 g/mol + 1.01 g/mol + 15.99 g/mol) = 60.05 g/mol.
Since acetic anhydride (C4H6O3) has twice the molar mass of acetic acid, the molar mass of acetic anhydride is:
2 x 60.05 g/mol = 120.10 g/mol.
Now, assuming the acetic anhydride fully converts to acetic acid, we can use the fact that 1 mole of acetic anhydride produces 2 moles of acetic acid.
Therefore, the number of moles of acetic acid added to the reaction is:
moles = (V mL x 1.05 g/mL) / (120.10 g/mol).
Please provide the volume of acetic anhydride added, and I can calculate the number of moles of acetic acid added.
To find the mass of acetic anhydride added to the reaction, we will need the volume of acetic anhydride that was added. Unfortunately, this information is not provided in the question. Once we have the volume, we can multiply it by the density of acetic anhydride (1.05 g/mL) to calculate the mass.
As for the number of moles of acetic acid added, I would require additional information about the reaction being performed. The reaction equation or the amount of another substance involved would be needed to determine the number of moles of acetic acid. Please provide more information to answer this part of the question.
5.25 g C4H6O3
0.0514 mol C2H4O2