Question

Из 300 м в кубе аммиака (н.у) получили 500 кг азотной кислоты. Вычислить выход продукта в процентах от теоретически возможного. Ответ есть (59%)

Answer 1

Синтез азотной кислоты идет в 3 стадии:
1 стадия:4NH3+5O2=4NO+6H2O
2 стадия:2NO+O2=2NO2
3 стадия:4NO2+2H2O+O2=4HNO3.
Суммарная реакция:
NH3+2O2=HNO3+H2O
1.n(NH3)=V/Vm=300000/22,4=13392,8571 моль
2.n(NH3)=n(NO)=n(NO2)=n(HNO3)=13392,8571 моль
3.m(HNO3,при теор.выходе)=n*M=13392,8571*63=843750 кг.
4.выход продукта=m(HNO3,при практ.выходе)/m(HNO3,при теор.выходе)=0,5925(59,25%).
Ответ:59,25%.

Answer 2

Calculating the Percentage Yield of the Reaction

To calculate the percentage yield of the reaction, we can use the following formula:

Percentage Yield = (Actual Yield / Theoretical Yield) x 100%

Given: - Initial amount of ammonia (NH3) = 300 m³ - Mass of nitric acid (HNO3) produced = 500 kg

First, we need to calculate the theoretical yield of nitric acid produced from the given amount of ammonia.

The balanced chemical equation for the reaction is: 4NH3 + 5O2 → 4NO + 6H2O

From the balanced equation, we can see that 4 moles of ammonia react to produce 4 moles of nitric oxide (NO).

Now, let's calculate the theoretical yield of nitric acid produced from the given amount of ammonia.

Calculating Theoretical Yield

1. Molar Mass of NH3 (Ammonia) - The molar mass of NH3 = 14.01 g/mol (N) + 3 * 1.01 g/mol (H) = 17.03 g/mol

2. Moles of NH3 - Moles of NH3 = (Given volume of NH3) / (Molar volume at NTP) - Moles of NH3 = (300 m³) / (22.4 m³/mol) = 13.39 moles

3. Moles of NO Produced - From the balanced equation, 4 moles of NH3 produce 4 moles of NO.

4. Molar Mass of HNO3 (Nitric Acid) - The molar mass of HNO3 = 1.01 g/mol (H) + 14.01 g/mol (N) + 3 * 16.00 g/mol (O) = 63.02 g/mol

5. Theoretical Yield of HNO3 - Theoretical Yield = (Moles of NO produced) * (Molar mass of HNO3) - Theoretical Yield = 13.39 moles * 63.02 g/mol = 842.88 g

Calculating Percentage Yield

Now that we have the theoretical yield, we can calculate the percentage yield using the formula:

Percentage Yield = (Actual Yield / Theoretical Yield) x 100%

Given: - Actual Yield = 500 kg = 500,000 g - Theoretical Yield = 842.88 g

Percentage Yield = (500,000 g / 842.88 g) x 100% ≈ 59%

Therefore, the percentage yield of the reaction is approximately 59%.