- #1
apache
when you equate the two formulas for ideal gases, one is evetually left with a formula to calculate the ke. of the ideal gas (3/2kt i think) how come the ke is independent of the mass of the molecule ?
Originally posted by apache
thanks guys,
i think i finally got it !
Originally posted by Tyger
The temperature is basically the mean energy per unit quantum, in this case atoms or molecules are the "quanta" involved, (this isn't the standard definition of quantum) and the pressure is the mean energy per unit volume...
In non-ideal gasses some of the energy is tied up in rotational modes, which is why they have differing ratios of specific heat.
The kinetic energy (KE) of ideal gases is calculated using the formula KE = 1/2 * m * v^2, where m is the mass of the gas molecule and v is its velocity.
No, the kinetic energy of ideal gases is independent of the mass of the gas molecules. This is because the formula for calculating KE takes into account both the mass and velocity of the molecules.
The kinetic energy of ideal gases is independent of molecule mass because the formula for KE takes into account both the mass and velocity of the molecules. This means that even if the mass of the molecules changes, the velocity changes in such a way that the overall kinetic energy remains constant.
As temperature increases, the average velocity of the gas molecules also increases. This results in an increase in the kinetic energy of the gas molecules. Therefore, there is a direct relationship between temperature and kinetic energy in ideal gases.
No, the kinetic energy of ideal gases cannot be measured directly. It is a theoretical concept that helps us understand the behavior of gases in certain conditions. However, it can be indirectly measured through other variables such as temperature, pressure, and volume.