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Question

According to the kinetic theory of gases, the pressure exerted by a gas is due to:

Mr. ANIL KUMAR.G · Accepted Answer

## CORE INFORMATION
✓ **Answer**: B
## CONCEPT FRAMEWORK
 **Primary Concept**: Kinetic Theory of Gases
 **Related Topics**: Pressure, Gas Molecules, Collisions
 **Prerequisites**: Understanding of gas molecules as tiny particles in constant random motion.
## SOLUTION PATHWAY
**Given Information**:
  The question asks about the cause of pressure in gases according to the kinetic theory.
**Method & Steps**:
 1. Understand the Kinetic Theory of Gases:  The kinetic theory states that gases consist of a large number of tiny particles (atoms or molecules) in constant, random motion. These particles are far apart compared to their size and exert negligible intermolecular forces.
  Reasoning: The pressure exerted by a gas is a macroscopic property arising from the microscopic behavior of its constituent particles.
 2. Consider the effect of collisions:  Gas molecules constantly collide with each other and with the walls of their container. These collisions exert a force on the walls.
  Working: The pressure is directly proportional to the number of collisions per unit time and the force exerted during each collision.  More frequent and forceful collisions lead to higher pressure.
 3. Relate collisions to pressure: The continuous bombardment of gas molecules on the container walls results in a net outward force, which is perceived as pressure.
  Result: The pressure of a gas is directly caused by the collisions of gas molecules with the walls of the container.
  Verification: This aligns perfectly with the ideal gas law, which relates pressure, volume, temperature, and the number of gas molecules.
 ## OPTION ANALYSIS
A :x: The weight of the gas molecules contributes negligibly to the pressure compared to the effect of collisions, especially for gases at low densities.
B ✓: This is the correct answer, as explained in the solution pathway.
C :x: Intermolecular forces are negligible in ideal gases, which are the basis of the kinetic theory.  Real gases exhibit some intermolecular forces, but these are not the primary cause of pressure.
D :x: While the size of gas molecules does influence the pressure (especially at high densities where the molecules occupy a significant fraction of the volume), the primary cause of pressure is the collisions of the molecules with the container walls.
 ## LEARNING AIDS
 **Common Mistakes**:
  1.Confusing pressure with the weight of the gas: The weight contributes minimally to the overall pressure.
  2.Overemphasizing intermolecular forces:  In ideal gases, these forces are assumed to be negligible.
 **Quick Tips**:
  1.Visualize gas molecules constantly bouncing off the walls of the container. 
  2.Remember that pressure is a consequence of many tiny impacts, not a single force.

Mr. ANIL KUMAR.G · Answer

The weight of the gas molecules

Mr. ANIL KUMAR.G · Answer

The correct Option is "Collisions of gas molecules with the walls of the container"

Mr. ANIL KUMAR.G · Answer

The intermolecular forces between gas molecules

Mr. ANIL KUMAR.G · Answer

The size of the gas molecules

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