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

Question

Which of the following assumptions of the kinetic theory of gases is NOT strictly true for real gases?

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: C
## CONCEPT FRAMEWORK
	**Primary Concept**: Kinetic Theory of Gases
	**Related Topics**: Ideal Gas Law, Intermolecular Forces, Real Gases
	**Prerequisites**: Basic understanding of the kinetic theory of gases and its assumptions.
## SOLUTION PATHWAY
**Given Information**:
	Assumptions of the kinetic theory of gases.
	Identification of assumptions not strictly true for real gases.
**Method & Steps**:
	1.	Review the assumptions of the kinetic theory of gases.
		Reasoning: The kinetic theory of gases makes several simplifying assumptions to describe gas behavior.
	2.	Identify the assumption that is not valid for real gases.
		Working: Real gases have intermolecular forces and their particles do have a finite size. The assumptions of kinetic theory are idealizations.
	3.	Select the assumption that does not hold for real gases.
		Result: The assumption that there are no intermolecular forces except during collisions is not true for real gases.
		Verification: Real gases experience attractive and repulsive forces between molecules, which affect their behavior.
 ## OPTION ANALYSIS
[A] :x: This assumption is generally true, even for real gases. The particles are very small relative to the distances between them.
[B] :x: Collisions are considered perfectly elastic for both ideal and real gases (in theory). While there might be some energy transfer in real collisions, the assumption holds reasonably well.
[C] ✓: This assumption is not strictly true for real gases. Real gas particles experience intermolecular forces (both attractive and repulsive) that influence their behavior, especially at higher pressures and lower temperatures.
[D] :x: This assumption is generally true for both ideal and real gases. The average kinetic energy of gas particles is directly proportional to the absolute temperature.
 ## LEARNING AIDS
	**Common Mistakes**:
		1.[Error 1]: Confusing ideal gas assumptions with real gas behavior. : [Understand that real gases deviate from ideal behavior due to intermolecular forces and finite particle size.]
		2.[Error 2]: Thinking that all assumptions of the kinetic theory are completely valid for all gases : [Recognize that the kinetic theory of gases is an idealization and real gases deviate from it.]
	**Quick Tips**:
		1.[Helpful shortcut]: Remember that real gas behavior deviates from ideal gas behavior because of intermolecular forces and finite particle volume.
		2.[Memory aid]: Think of real gases as having 'sticky' particles that interact, unlike the perfectly independent particles assumed in the kinetic theory.

Mr. S M HUSSAIN · Answer

Gas consists of a large number of very small particles that are far apart relative to their size.

Mr. S M HUSSAIN · Answer

The collisions between gas particles and with the walls of the container are perfectly elastic.

Mr. S M HUSSAIN · Answer

The correct Option is "There are no intermolecular forces between the particles except during collisions."

Mr. S M HUSSAIN · Answer

The average kinetic energy of the gas particles is proportional to the absolute temperature of the gas.

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