What is the difference between BOYLE'S LAW and BOYLE'S TEMPERATURE ? Define it.
Answers
Answered by
11
Boyle's law is a gas law. Boyle's law states that at a fixed temperature for a given amount of gas, the volume of the gas is inversely proportional to the pressure. Or, the pressure is inversely proportional to the volume.
P ∞ 1/V or P V = constant , at constant T.
Or, P₁ * V₁ = P₂ * V₂
This law was proposed by Robert Boyle in 1662. Ideal gases follow this law. In reality at low pressures, this law is valid very well. At high pressures, there is a deviation by real gases from the ideal gas behaviour.
==============
Boyle temperature :
In reality gases are not ideal. There are attractive forces due to gravitational forces between the molecules. There are also repulsive forces between molecules due to electromagnetic and other properties of atoms and subatomic particles.
Boyle Temperature for a gas is that temperature at which the real gas behaves almost as an ideal gas. At this temperature the attractive forces and the repulsive forces among molecules nearly cancel out. The deviation from ideal gas behaviour is very negligible over a wide range of pressures.
Then P = nRT/V is valid for a considerable range of Pressure P.
At Boyle temperature the compressibility factor of the gas Z is almost 1. It does not vary with pressure. At Boyle temperature Boyle's law is obeyed very closely by the real gases.
The Vander Wall's gas equation reduces to Ideal gas equation, as Vander Wall forces are nullified by the effect of temperature.
P ∞ 1/V or P V = constant , at constant T.
Or, P₁ * V₁ = P₂ * V₂
This law was proposed by Robert Boyle in 1662. Ideal gases follow this law. In reality at low pressures, this law is valid very well. At high pressures, there is a deviation by real gases from the ideal gas behaviour.
==============
Boyle temperature :
In reality gases are not ideal. There are attractive forces due to gravitational forces between the molecules. There are also repulsive forces between molecules due to electromagnetic and other properties of atoms and subatomic particles.
Boyle Temperature for a gas is that temperature at which the real gas behaves almost as an ideal gas. At this temperature the attractive forces and the repulsive forces among molecules nearly cancel out. The deviation from ideal gas behaviour is very negligible over a wide range of pressures.
Then P = nRT/V is valid for a considerable range of Pressure P.
At Boyle temperature the compressibility factor of the gas Z is almost 1. It does not vary with pressure. At Boyle temperature Boyle's law is obeyed very closely by the real gases.
The Vander Wall's gas equation reduces to Ideal gas equation, as Vander Wall forces are nullified by the effect of temperature.
kvnmurty:
:-)
Thanks
Answered by
0
Answer:
idk jufmmgydkyekthegdhtjryegdmhmdhh af f.fj
Similar questions