The Question is from neet-chemistry basic-chemistry-concepts concentration-methods, and it was created by the author A.RAMA NAGESWARARAO

Question

When one mole of ${\rm{KMn}}{{\rm{O}}_4}$ reacts with $HCl$, the volume of chlorine liberated at  $NTP$  will be:

A.RAMA NAGESWARARAO · Accepted Answer

## CORE INFORMATION
✓ **Answer**: D
## CONCEPT FRAMEWORK
	**Primary Concept**: Stoichiometry of Redox Reactions
	**Related Topics**: Balancing Redox Reactions, Molar Volume at NTP, Ideal Gas Law
	**Prerequisites**: Knowledge of redox reactions, balancing chemical equations, and molar volume at NTP.
## SOLUTION PATHWAY
**Given Information**:
	* 1 mole of KMnO4 reacts with HCl
	* We need to find the volume of chlorine (Cl2) liberated at NTP
**Method & Steps**:
	1. **Write and Balance the Redox Reaction:**
	   The unbalanced reaction is:
       $KMnO_4 + HCl ightarrow KCl + MnCl_2 + H_2O + Cl_2$
      The balanced reaction is:
      $2KMnO_4 + 16HCl ightarrow 2KCl + 2MnCl_2 + 8H_2O + 5Cl_2$
	   Reasoning: Balancing the redox reaction using oxidation number change method.
	2. **Determine the moles of $Cl_2$ produced**: 
	   From the balanced equation, 2 moles of $KMnO_4$ produce 5 moles of $Cl_2$.
	   Therefore, 1 mole of $KMnO_4$ will produce $\frac{5}{2}$ moles of $Cl_2$, which is 2.5 moles of $Cl_2$.
	   Working: Mole ratio from the balanced equation.
	   Key Point: Using stoichiometric coefficients correctly.
	3. **Calculate the volume of $Cl_2$ at NTP**: 
	   At NTP (Normal Temperature and Pressure), 1 mole of any gas occupies 22.4 liters.
	   Therefore, 2.5 moles of $Cl_2$ will occupy $2.5 	imes 22.4$ liters.
	   $2.5 	imes 22.4 = 56$ liters.
	   Result: Volume of chlorine gas liberated is 56 liters.
	   Verification: Dimensional analysis and unit consistency.
 ## OPTION ANALYSIS
[A] :x: This would be the volume for 0.5 moles of Cl2, not 2.5.
[B] :x: This is the volume for 1 mole of gas, not 2.5 moles of Cl2.
[C] :x: This is the volume for 2 moles of gas, not 2.5 moles of Cl2.
[D] ✓: This is the correct volume calculated based on the stoichiometry and molar volume at NTP.
 ## LEARNING AIDS
	**Common Mistakes**:
		1.[Error 1]: Incorrectly balancing the redox reaction. [How to avoid]: Use the oxidation number change method systematically.
		2.[Error 2]: Forgetting to use the molar volume at NTP. [How to avoid]: Remember that 1 mole of any gas occupies 22.4 liters at NTP.
	**Quick Tips**:
		1.[Helpful shortcut]: Always start with a balanced chemical equation.
		2.[Memory aid]: Remember the molar volume of a gas at NTP (22.4L).

A.RAMA NAGESWARARAO · Answer

11.2 litre

A.RAMA NAGESWARARAO · Answer

22.4 litre

A.RAMA NAGESWARARAO · Answer

44.8 litre

A.RAMA NAGESWARARAO · Answer

The correct Option is "56.0 litre"

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