An unknown compound has the following chemical formula NxO3 where x stands for a whole number measurements also show that a cert
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<u>Answer:</u> The theoretical yield of acetanilide is 6.5 grams.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For aniline:</u>
Given mass of aniline = (We know that:
)
Molar mass of aniline = 93.13 g/mol
Putting values in equation 1, we get:
- <u>For acetic anhydride:</u>
To calculate the mass of acetic anhydride, we use the equation:
Volume of acetic anhydride =
Density of acetic anhydride = 1.08 g/mL
Putting values in above equation:
Given mass of acetic anhydride = 6.08 g
Molar mass of acetic anhydride = 102.1 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of aniline and acetic anhydride follows:
By Stoichiometry of the reaction:
1 mole of aniline reacts with 1 mole of acetic anhydride
So, 0.048 moles of aniline will react with = of acetic anhydride
As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.
Thus, aniline is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of aniline produces 1 mole of acetanilide
So, 0.048 moles of aniline will produce = of acetanilide
Now, calculating the theoretical yield of acetanilide by using equation 1:
Moles of acetanilide = 0.048 moles
Molar mass of acetanilide = 135.17 g/mol
Putting values in equation 1, we get:
Hence, the theoretical yield of acetanilide is 6.5 grams.