If you used 0.155 mL of acetic anhydride, and 0.169 g of p-aminophenol what was the limiting reagent?

Choice is either:
1. acetic anhydride
or
2. p-aminophenol

________mol?
How many moles of the non-limiting reageant remained after the reaction was complete?

To determine the limiting reagent, we need to compare the number of moles of each reactant and calculate the mole ratio based on the balanced chemical equation.

First, we need to convert the given amounts of acetic anhydride and p-aminophenol into moles:

Molar mass of acetic anhydride (CH3CO)2O: 102.09 g/mol
Number of moles of acetic anhydride = 0.155 mL (convert to grams) / molar mass
Number of moles of acetic anhydride = 0.155 g / 102.09 g/mol = 0.00152 mol

Molar mass of p-aminophenol (C6H7NO): 109.13 g/mol
Number of moles of p-aminophenol = 0.169 g / 109.13 g/mol = 0.00155 mol

Next, we determine the mole ratio between acetic anhydride and p-aminophenol based on the balanced chemical equation. Let's assume the balanced equation is:

2(CH3CO)2O + C6H7NO -> 2C8H9NO2 + CH3COOH

From the equation, we can see that the mole ratio between acetic anhydride and p-aminophenol is 2:1. This means that for every 2 moles of acetic anhydride, 1 mole of p-aminophenol is required.

Since the mole ratio is 2:1, and the actual mole ratio of acetic anhydride to p-aminophenol is 0.00152 mol / 0.00155 mol ≈ 0.98:1, we can conclude that acetic anhydride is the limiting reagent.

Therefore, the limiting reagent is 1. acetic anhydride.

Now, to calculate the number of moles of the non-limiting reagent remaining after the reaction, we need to determine the excess amount of the non-limiting reagent.

In this case, p-aminophenol is the non-limiting reagent.
Since p-aminophenol is in excess, all of the acetic anhydride will be consumed, and there will be some p-aminophenol left over.

The amount of p-aminophenol remaining can be calculated by subtracting the moles of p-aminophenol reacted from the initial moles:

Initial moles of p-aminophenol = 0.00155 mol
Moles of p-aminophenol reacted = (0.00152 mol of acetic anhydride) * (1 mol of p-aminophenol / 2 mol of acetic anhydride) = 0.00076 mol

Remaining moles of p-aminophenol = Initial moles - Moles reacted
Remaining moles of p-aminophenol = 0.00155 mol - 0.00076 mol = 0.00079 mol

Therefore, after the reaction is complete, 0.00079 moles of p-aminophenol will remain.

To determine the limiting reagent in a chemical reaction, you need to compare the number of moles of each reactant and their stoichiometric ratios.

First, let's calculate the number of moles for each reactant using their respective molar masses:

Molar mass of acetic anhydride (C4H6O3):
C = 4.01 g/mol,
H = 1.01 g/mol (x 6),
O = 16.00 g/mol (x 3).

Total molar mass of acetic anhydride = (4.01 x 4) + (1.01 x 6) + (16.00 x 3) = 102.08 g/mol.

Given that you used 0.155 mL of acetic anhydride and assuming a density of 1 g/mL, we can convert the volume to grams:
0.155 mL x 1 g/mL = 0.155 g.

Now, let's calculate the number of moles of acetic anhydride:
Moles = Mass / Molar mass = 0.155 g / 102.08 g/mol.

Molar mass of p-aminophenol (C6H7NO):
C = 12.01 g/mol (x 6),
H = 1.01 g/mol (x 7),
N = 14.01 g/mol,
O = 16.00 g/mol.

Total molar mass of p-aminophenol = (12.01 x 6) + (1.01 x 7) + (14.01) + (16.00) = 109.13 g/mol.

Given that you used 0.169 g of p-aminophenol:

Moles = Mass / Molar mass = 0.169 g / 109.13 g/mol.

Now compare the number of moles of acetic anhydride and p-aminophenol to determine the limiting reagent. The reactant that produces fewer moles of product is the limiting reagent.

Next, calculate the amount of product formed using the stoichiometric ratio between acetic anhydride and p-aminophenol, which is determined by the balanced chemical equation of the reaction. The balanced equation is needed to calculate the moles of the non-limiting reactant that remained after the reaction.

Please provide the balanced chemical equation for the reaction between acetic anhydride and p-aminophenol so that we can determine the limiting reagent and the number of moles of the non-limiting reagent remaining.