Question

При взаимодействии с аммиаком 190 г бромуксусной кислоты, содержащей 2% примеси, образовано 75,3 г аминоуксусной кислоты. Определите выход продукта реакции от теоретически возможного.

Answer 1

Ответконтрольная по химии?

Объяснение:

Answer 2

Reaction Stoichiometry

To determine the theoretical yield of the reaction, we need to understand the stoichiometry of the reaction between ammonia (NH3) and bromoacetic acid (C2H3BrO2). The balanced equation for the reaction is as follows:

NH3 + C2H3BrO2 -> NH2CH2COOH + HBr

According to the given information, 190 g of bromoacetic acid (C2H3BrO2) with 2% impurities reacted to form 75.3 g of aminomethylcarboxylic acid (NH2CH2COOH).

Calculating Theoretical Yield

To calculate the theoretical yield of the reaction, we can use the stoichiometry of the balanced equation. The molar mass of bromoacetic acid (C2H3BrO2) is 138.96 g/mol, and the molar mass of aminomethylcarboxylic acid (NH2CH2COOH) is 75.07 g/mol.

1 mole of bromoacetic acid (C2H3BrO2) reacts to form 1 mole of aminomethylcarboxylic acid (NH2CH2COOH). Therefore, the molar ratio between the two compounds is 1:1.

We can calculate the number of moles of bromoacetic acid used in the reaction as follows:

Number of moles of bromoacetic acid = Mass of bromoacetic acid / Molar mass of bromoacetic acid Number of moles of bromoacetic acid = 190 g / 138.96 g/mol ≈ 1.366 mol

Since the molar ratio between bromoacetic acid and aminomethylcarboxylic acid is 1:1, the number of moles of aminomethylcarboxylic acid formed will be the same as the number of moles of bromoacetic acid used.

Therefore, the theoretical yield of aminomethylcarboxylic acid can be calculated as follows:

Theoretical yield of aminomethylcarboxylic acid = Number of moles of aminomethylcarboxylic acid * Molar mass of aminomethylcarboxylic acid Theoretical yield of aminomethylcarboxylic acid = 1.366 mol * 75.07 g/mol ≈ 102.5 g

Determining the Percentage Yield

To determine the percentage yield, we can use the following formula:

Percentage yield = (Actual yield / Theoretical yield) * 100

Given that the actual yield of aminomethylcarboxylic acid is 75.3 g and the theoretical yield is approximately 102.5 g, we can calculate the percentage yield as follows:

Percentage yield = (75.3 g / 102.5 g) * 100 ≈ 73.5%

Therefore, the percentage yield of the reaction is approximately 73.5% of the theoretical yield.

Note: The information provided is based on the given data and assumes that the reaction proceeds according to the balanced equation.