Question

Для получения азотной кислоты промышленным способом использовали аммиак объемом 44.8 л (при н.у) и другие необходимые вещества. В результате была получена 100%-ная азотная кислота массой 120 кг. Определите, какой это составляет выход в процентах от теоретического. Какую массу раствора с массовой долей 0.7 можно приготовить из реально полученной азотной кислоты? (Для расчета используйте схему NH30->HNO3 ​

Answer 1

Ответ:

44,8 / 22,4 = 2 моль

4NH3 + 5О2 → 4NO + 6Н2О

2NO + О2 → 2NO2

NO2 + H20 => HNO3

HNO3 = 0,5 моль

120000/ 63(HNO3) = 1904,76 моль

Объяснение:

Answer 2

Calculation of Yield Percentage

To determine the yield percentage of the nitric acid obtained, we need to compare the actual mass of the nitric acid produced with the theoretical mass that could have been obtained.

Given: - Volume of ammonia used: 44.8 L (at standard temperature and pressure) - Mass of 100% nitric acid obtained: 120 kg

To calculate the theoretical mass of nitric acid that could have been obtained, we need to use the balanced chemical equation for the reaction:

4NH3 + 5O2 → 4HNO3 + 6H2O

From the equation, we can see that 4 moles of ammonia react to produce 4 moles of nitric acid. The molar mass of ammonia (NH3) is approximately 17 g/mol, and the molar mass of nitric acid (HNO3) is approximately 63 g/mol.

Using the given volume of ammonia, we can calculate the number of moles of ammonia used:

Number of moles of ammonia = (volume of ammonia / molar volume at STP) = (44.8 L / 22.4 L/mol) = 2 moles

Since the reaction stoichiometry is 4:4, the number of moles of nitric acid produced is also 2 moles.

The theoretical mass of nitric acid that could have been obtained is then:

Theoretical mass of nitric acid = (number of moles of nitric acid * molar mass of nitric acid) = (2 moles * 63 g/mol) = 126 g

To calculate the yield percentage, we can use the formula:

Yield percentage = (actual mass of nitric acid obtained / theoretical mass of nitric acid) * 100

Substituting the given values:

Yield percentage = (120 kg / 126 g) * 100 = 95.24%

Therefore, the yield of nitric acid obtained is approximately 95.24% of the theoretical yield.

Calculation of Mass of Solution with a Mass Fraction of 0.7

To calculate the mass of a solution with a mass fraction of 0.7 that can be prepared from the obtained nitric acid, we need to use the definition of mass fraction:

Mass fraction = (mass of solute / mass of solution)

Given: - Mass fraction of the solution: 0.7

Let's assume the mass of the solution to be x grams.

The mass of the solute (nitric acid) can be calculated as:

Mass of solute = (mass fraction of solute * mass of solution) = (0.7 * x)

Since the mass of the solute is the same as the mass of the obtained nitric acid (120 kg), we can equate the two:

0.7 * x = 120 kg

Converting the mass of the solution to grams:

x = (120 kg * 1000 g/kg) / 0.7 = 171,428.57 g

Therefore, the mass of the solution with a mass fraction of 0.7 that can be prepared from the obtained nitric acid is approximately 171,428.57 grams.

Note: The calculation assumes that the mass fraction of the nitric acid remains constant when preparing the solution.