Question

30 балів Англійський хімік технолог Генрі Дікон у 1867 році розробив спосіб добування хлору шляхом каталітичного окислення хлороводню киснем повітря при температурі 400o С в присутності каталізатора – купрум (ІІ) хлориду: CuCl2 + 4HCl + O2 = 2Cl2 + 2H2O. Цей метод отримав назву реакції Дікона, а промислова технологія – процес Дікона. Обчисліть, який об’єм хлору можна добути, в ході процесу Дікона з 100 (кг) хлороводню і 16 (мл) кисню.

Answer 1

Ответ:

              100      16

CuCl2 + 4HCl + O2 = 2Cl2 + 2H2O.

               2.7                 1.35

n(HCl) = 100/36.5 = 2.7 моль

n(Cl2) = n(HCl) / 2 = 1.35 моль

V(Cl2) = Vm * n(Cl2)

V(Cl2) = 22.4 * 1.35 = 30.24 л

Объяснение:

Answer 2

Henry Deacon's Chlorine Production Process

English chemist and technologist Henry Deacon developed a method for extracting chlorine through the catalytic oxidation of hydrogen chloride with oxygen in the presence of a catalyst – cupric (II) chloride: CuCl2 + 4HCl + O2 = 2Cl2 + 2H2O at a temperature of 400°C. This method is known as the Deacon reaction, and the industrial technology is referred to as the Deacon process.

Calculating the Volume of Chlorine Produced

To calculate the volume of chlorine produced during the Deacon process, we can use the given amounts of hydrogen chloride and oxygen.

Given: - 100 kg of hydrogen chloride - 16 ml of oxygen

Calculation Steps

1. Convert the mass of hydrogen chloride to moles using the molar mass of HCl. 2. Use the stoichiometry of the reaction to determine the moles of chlorine produced. 3. Convert the moles of chlorine to volume using the ideal gas law.

Calculation

1. Convert 100 kg of hydrogen chloride to moles: - Molar mass of HCl = 1.00794 (H) + 35.453 (Cl) = 36.46094 g/mol - Moles of HCl = (100,000 g) / (36.46094 g/mol) = 2743.29 moles

2. Use stoichiometry to determine moles of chlorine produced: - From the balanced equation: 4 moles of HCl produce 2 moles of Cl2 - Moles of Cl2 produced = (2743.29 moles HCl) / 4 * 2 = 1371.65 moles

3. Convert moles of chlorine to volume at 400°C and 1 atm pressure: - Using the ideal gas law: PV = nRT - Assuming T = 400°C = 673.15 K and P = 1 atm - V = (1371.65 moles * 0.0821 L*atm/mol*K * 673.15 K) / 1 atm = 76,073.6 L

Answer

The volume of chlorine that can be produced during the Deacon process from 100 kg of hydrogen chloride and 16 ml of oxygen is approximately 76,073.6 liters.