The Question is from neet-chemistry chemical-thermodynamics , and it was created by the author A.RAMA NAGESWARARAO

Question

A real gas most closely approaches ideal behavior under which of the following conditions?

A.RAMA NAGESWARARAO · Accepted Answer

## CORE INFORMATION
✓ **Answer**: A
## CONCEPT FRAMEWORK
 **Primary Concept**: Ideal Gas Law vs. Real Gas Behavior
 **Related Topics**: Compressibility factor, van der Waals equation
 **Prerequisites**: Understanding of ideal gas law ($PV = nRT$) and the factors that cause deviations from ideal behavior (intermolecular forces and molecular volume).
## SOLUTION PATHWAY
**Given Information**:
The question asks under what conditions a real gas behaves most like an ideal gas.
**Method & Steps**:
1. Understanding Ideal Gas Behavior:
  Reasoning: An ideal gas is a theoretical gas composed of particles with negligible volume and no intermolecular forces.  Real gases deviate from this ideal behavior, especially at high pressures and low temperatures.
  Formula/Rule: $PV = nRT$ (Ideal gas law)
2. Effects of Pressure and Temperature:
  Working: High pressure forces gas molecules closer together, increasing the importance of intermolecular forces and molecular volume. Low temperature reduces the kinetic energy of molecules, making intermolecular forces more significant.
  Key Point:  Low pressure allows gas molecules to be far apart, minimizing the effect of both intermolecular forces and molecular volume. High temperature increases kinetic energy, making intermolecular forces less impactful.
3. Optimal Conditions:
  Result: Low pressure and high temperature minimize deviations from ideal gas behavior.
  Verification: Under these conditions, the gas molecules are far apart, move rapidly, and intermolecular interactions are negligible, closely approximating the conditions of an ideal gas.
 ## OPTION ANALYSIS
A ✓: Low pressure and high temperature: This condition minimizes intermolecular attractions and the effects of molecular volume, leading to behavior closest to an ideal gas.
B :x: High pressure and low temperature:  Both these conditions enhance deviations from ideal behavior.
C :x: High pressure and high temperature: High pressure is the major cause of deviation from ideal behavior.
D :x: Low pressure and low temperature: Low temperature enhances the effect of intermolecular forces.
 ## LEARNING AIDS
 **Common Mistakes**:
  1.Confusing the effects of pressure and temperature: Remember that high pressure and low temperature lead to significant deviations from ideal behavior.
  2.Overlooking the role of intermolecular forces: These forces are the primary reason why real gases deviate from ideal behavior.
 **Quick Tips**:
  1.Think about how pressure and temperature affect the distance between gas molecules and the strength of intermolecular forces.
  2.Remember that ideal gas behavior is an approximation, and real gases only approach ideal behavior under specific conditions.

A.RAMA NAGESWARARAO · Answer

The correct Option is "Low pressure and high temperature"

A.RAMA NAGESWARARAO · Answer

High pressure and low temperature

A.RAMA NAGESWARARAO · Answer

High pressure and high temperature

A.RAMA NAGESWARARAO · Answer

Low pressure and low temperature

NEET Chemistry States Of Matter MCQs

Select Topic

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

NEET Subjects

Our Bots

Company