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rogerk8 said:Is it correct to say that below this critical temperature gases may be converted into liquid?
It is only below the critical temperature that they can. Check out "supercritical fluid".
rogerk8 said:Is it correct to say that below this critical temperature gases may be converted into liquid?
The average translational kinetic energy is NkT/2 for each translational degree of freedom, so <KE> = 3NkT/2rogerk8 said:Jesus, I know nothing but please consider this:
[tex]U=KE+PE[/tex]
and
[tex]KE=kT≈\frac{mv^2}{2}[/tex]
and
[tex]\frac{PV}{N}=kT[/tex]
Then
[tex]U=kT+kT[/tex]
?
Do you have a specific question about PE and pressure?rogerk8 said:Thank you once again Andrew Mason!
I am thankful for all your help!
Now I know that there is a kinetic energy of NkT/2 per degree of freedom and that this is associated with potential energy as well.
My brand new understanding of internal energy is thus
[tex]U=KE+PE=fNkT/2[/tex]
But what about PE and pressure?
Roger
Andrew Mason said:Do you have a specific question about PE and pressure?
First of all you have to have a non-ideal gas with attractive forces between molecules. For such a gas PE increases with volume (as the space between molecules grows, on average, so does PE). If T remains constant (i.e. KE is constant) what happens to the pressure? (hint: how is pressure related to the rate at which molecules change momentum in striking the container walls? If KE is constant, but the distance between walls increases, what happens to the frequency of molecules colliding with the wall?).
AM
Pressure and the rate of momentum change in a gas are directly related. As pressure increases, the molecules in the gas become more tightly packed and collide with each other more frequently, resulting in a higher rate of momentum change. This is known as the ideal gas law, which states that pressure is directly proportional to the number of collisions and therefore the rate of momentum change.
Yes, the ideal gas law equation, PV = nRT, represents the relationship between pressure (P) and the rate of momentum change (V) in a gas. This equation combines Boyle's Law, which states that pressure and volume are inversely proportional, and Charles's Law, which states that volume and temperature are directly proportional.
Temperature also plays a role in the relationship between pressure and the rate of momentum change in a gas. As temperature increases, the molecules in the gas have more energy and move faster, resulting in more frequent collisions and a higher rate of momentum change. This is reflected in the ideal gas law equation, where temperature (T) is directly proportional to the rate of momentum change (V).
Yes, both pressure and the rate of momentum change in a gas can be manipulated. By changing the volume, temperature, or number of molecules in a gas, the pressure and rate of momentum change can be altered. For example, increasing the temperature of a gas will result in a higher pressure and rate of momentum change.
Pressure is directly related to the kinetic energy of gas molecules. As pressure increases, the average kinetic energy of the molecules also increases. This is because as pressure increases, the molecules have less space to move and therefore collide with each other more frequently, resulting in an increase in kinetic energy. This relationship is also reflected in the ideal gas law equation, where pressure (P) is directly proportional to the temperature (T).