Why do real gases behave as a ideal gas at high temperature and low pressure only give reason
Asked by venkat
20th December 2017,
2:38 PM
Answered by Expert
Answer:
The two assumptions in the ideal gas are
1. volume occupied by an individual molecule is very negligible as compared to the volume occupied by the gas as a whole.
2. The molecules do not exert any attractive forces on each other.
At high temperature and pressure, gases occupy even more amount of volume because of which the intermolecular distance increases and application of force on each other because more difficult.
Answered by Expert
20th December 2017,
5:12 PM
Rate this answer
- 1
- 2
- 3
- 4
- 5
- 6
- 7
- 8
- 9
- 10
You have rated this answer /10
Your answer has been posted successfully!
RELATED STUDY RESOURCES :
Browse free questions and answers by Chapters
- 1 Thermodynamics
- 2 Gravitation
- 3 Electromagnetic Waves
- 4 Communication Systems
- 5 Laws of Motion
- 6 Current Electricity
- 7 Work, Energy and Power
- 8 Kinematics
- 9 Physics and Measurement
- 10 Rotational Motion
- 11 Properties of Solids and Liquids
- 12 Kinetic Theory of Gases
- 13 Oscillations and Waves
- 14 Electrostatics
- 15 Magnetic Effects of Current and Magnetism
- 16 Electromagnetic Induction and Alternating Currents
- 17 Optics
- 18 Dual Nature of Matter and Radiation
- 19 Atoms and Nuclei
- 20 Electronic Devices
Trending Tags
Latest Questions
JEE Main Mathematics
Asked by amaladelsingh
28th October 2020,
10:24 PM
CBSE X Biology
Asked by reenacharan2008
28th October 2020,
9:11 PM
