The Question is from neet-chemistry , and it was created by the author Mr. S M HUSSAIN

Question

Cuprous chloride is obtained from cupric chloride:

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: C
## CONCEPT FRAMEWORK
	**Primary Concept**: Reduction of Cupric Chloride to Cuprous Chloride
	**Related Topics**: Redox reactions, Copper chemistry, Chemical reactions
	**Prerequisites**: Knowledge of copper compounds and their reactions.
## SOLUTION PATHWAY
**Given Information**:
	* Starting material: Cupric chloride (CuCl2)
	* Target product: Cuprous chloride (CuCl)
**Method & Steps**:
	1. **Understanding the Reaction**: Cuprous chloride has a lower oxidation state of copper (+1) compared to cupric chloride (+2). This means a reduction reaction is required.
		Reasoning: Cupric chloride needs to gain electrons to become cuprous chloride.
	2. **Analyzing the Options**:
		* A. Heating with chlorine: Chlorine is an oxidizing agent and would not reduce copper. This is incorrect.
		* B. Electrolysis of cupric chloride in HCl: While electrolysis can achieve reduction, the reaction isn't specific to producing cuprous chloride, and typically involves the formation of copper metal. This is incorrect.
		* C. Heating with conc. HCl and copper turnings: Copper turnings will reduce cupric chloride in the presence of HCl. The reaction is:
		  $CuCl_2 + Cu + 2HCl  ightarrow 2CuCl + H_2$
		  This is the correct process for preparing CuCl
		* D. Passing H2 over CuCl2: Hydrogen gas can act as a reducing agent. However, this is not a common method for the synthesis of CuCl. This is incorrect.
	3. **Final Step**: The correct answer is option C.
		Result: Option C is correct.
		Verification: Consistent with known chemical reactions.
 ## OPTION ANALYSIS
[A] :x: Chlorine will not reduce copper.
[B] :x: Electrolysis produces copper metal.
[C] ✓: Copper turnings reduce Cupric chloride to Cuprous chloride in HCl.
[D] :x: Hydrogen is not the preferred method for this synthesis.
 ## LEARNING AIDS
	**Common Mistakes**:
		1. Confusing oxidizing and reducing agents: Understand that chlorine is an oxidizer and will not reduce copper.
		2. Not knowing the common methods of synthesizing cuprous chloride: Remember that copper metal is a reducing agent and can be used to reduce cupric chloride.
	**Quick Tips**:
		1. Focus on the change in oxidation state. Cupric (+2) to cuprous (+1) implies reduction.
		2. Remember that copper metal can act as a reducing agent.

Mr. S M HUSSAIN · Answer

By heating cupric chloride with chlorine

Mr. S M HUSSAIN · Answer

By the electrolysis of cupric chloride containing HCl

Mr. S M HUSSAIN · Answer

The correct Option is "By heating cupric chloride with conc. HCl and copper turnings"

Mr. S M HUSSAIN · Answer

By passing ${{\rm{H}}_2}\;$  over ${\rm{CuC}}{{\rm{l}}_2}$

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