Question

Identify the reaction related to Deacon's process

• A. \(2\text{H}_2\text{O} + 2\text{Cl}_2 \xrightarrow{\text{sunlight}} 4\text{HCl} + \text{O}_2\)
• B. \(4\text{HCl} + \text{O}_2 \xrightarrow[723\text{K}]{\text{CuCl}_2} 2\text{Cl}_2 + 2\text{H}_2\text{O}\)
• C. \(2\text{NaCl} + \text{H}_2\text{SO}_4 \xrightarrow{823\text{K}} \text{Na}_2\text{SO}_4 + 2\text{HCl}\)
• D. \(\text{Na}_2\text{S}_2\text{O}_3 + \text{Cl}_2 + \text{H}_2\text{O} \rightarrow \text{Na}_2\text{SO}_4 + 2\text{HCl} + \text{S}\)

Hint:

Remember: Deacon's Process \(\rightarrow\) Manufacture of Chlorine. Catalyst \(\rightarrow\) \(\text{CuCl}_2\). Reactants \(\rightarrow\) \(\text{HCl} + \text{O}_2\).

Answer 1

The Correct Option is B

Step 1: Understanding Deacon's Process:
Deacon's process is a well-known industrial method for the manufacture of Chlorine gas (\(\text{Cl}_2\)). It involves the oxidation of hydrogen chloride gas by atmospheric oxygen.
Step 2: Reaction Conditions:
The reaction typically takes place at a temperature of about \(723\text{ K}\) (\(450^\circ\text{C}\)) in the presence of a catalyst, Cupric Chloride (\(\text{CuCl}_2\)).
Step 3: Chemical Equation:
The balanced chemical equation is: \[ 4\text{HCl} + \text{O}_2 \xrightarrow{\text{CuCl}_2, 723\text{K}} 2\text{Cl}_2 + 2\text{H}_2\text{O} \] This matches Option (B). Final Answer:
Option (B).