Question

5.8 g of Aniline is converted into benzanilide with some reaction sequences. Calculate the mass of benzanilide formed, if percentage yield of reaction is 82%. \[ \text{Ph} - \text{COCl} + \text{PhNH}_2 \xrightarrow{\text{Py}} \text{Benzanilide} \]

Hint:

To calculate the actual yield of a reaction, multiply the theoretical yield by the percentage yield.

Answer 1

Correct Answer: 3

Step 1: Calculate the molar mass of aniline.
The molar mass of aniline (C\(_6\)H\(_5\)NH\(_2\)) is 93 g/mol. Step 2: Calculate the moles of aniline.
The moles of aniline used are: \[ \text{moles of aniline} = \frac{5.8}{93} = 0.0624 \, \text{mol}. \] Step 3: Use the stoichiometry of the reaction.
From the reaction, 1 mole of aniline produces 1 mole of benzanilide. Therefore, the theoretical mass of benzanilide is: \[ \text{theoretical mass} = 0.0624 \times 226 = 14.1 \, \text{g}. \] Step 4: Apply the percentage yield.
The actual mass is calculated using the percentage yield: \[ \text{actual mass} = 14.1 \times \frac{82}{100} = 6.5 \, \text{g}. \] Final Answer: \[ \boxed{6.5 \, \text{g}}. \]