Question

Найдите массу азотной кислоты полученной взаимодействием 460г диаксида азота и кислорода. Практический выход кислоты равен 80% от теоретически возможного.

Answer 1

привет))

расчитаем количество NO2=460/46=10(моль);

расчитаем массу HNO3=10моль*63г/моль=630(г)

масса HNO3=630/80*100=787.5(г) это ответ

Answer 2

Calculating the Mass of Nitric Acid Produced

To calculate the mass of nitric acid produced, we can use the given information about the reaction and the practical yield.

Given: - Mass of dinitrogen tetroxide (N2O4) = 460g - Practical yield of the reaction = 80%

The balanced chemical equation for the reaction is: N2O4 + O2 → 2HNO3

From the balanced equation, we can see that 1 mole of N2O4 reacts with 1 mole of O2 to produce 2 moles of HNO3.

Calculating the Theoretical Yield

First, we need to calculate the number of moles of N2O4: - The molar mass of N2O4 is 92.02 g/mol. - Number of moles of N2O4 = Mass of N2O4 / Molar mass of N2O4 - Number of moles of N2O4 = 460g / 92.02 g/mol - Number of moles of N2O4 = 5 moles

According to the balanced chemical equation, 1 mole of N2O4 produces 2 moles of HNO3. Therefore, the theoretical yield of HNO3 can be calculated as: - Theoretical yield of HNO3 = 2 * Number of moles of N2O4 - Theoretical yield of HNO3 = 2 * 5 moles - Theoretical yield of HNO3 = 10 moles

Calculating the Mass of Nitric Acid Produced

Now, we can calculate the mass of nitric acid produced based on the theoretical yield and the practical yield: - Mass of HNO3 = Theoretical yield of HNO3 * Molar mass of HNO3 - The molar mass of HNO3 is 63.01 g/mol. - Mass of HNO3 = 10 moles * 63.01 g/mol - Mass of HNO3 = 630.1g

Finally, applying the practical yield: - Actual mass of nitric acid produced = Practical yield * Theoretical mass of nitric acid - Actual mass of nitric acid produced = 80% * 630.1g - Actual mass of nitric acid produced = 504.08g

Therefore, the mass of nitric acid produced is approximately 504.08 grams.