In an ideal gas of monatomic particles, the average kinetic energy is
<K>=(3/2)*k*T
In a more general ideal gas, the average energy of each particle is
<K>=(d/2)*k*T
where d is the number of degrees of freedom. There isn't a clear distinction between kinetic and potential energy for general degrees of freedom.
For normal (non-negative) temperatures, as temperature increases, so does energy. The exact relation depends on the entropy of the system.
T=dU/dS, where d is the partial derivative.
http://en.wikipedia.org/wiki/Equipartition_theorem
http://en.wikipedia.org/wiki/Ideal_gas
The expression for gas pressure developed from kinetic theory relates pressure and volume to the average molecular kinetic energy. Comparison with the ideal gas law leads to an expression for temperature sometimes referred to as the kinetic temperature.
It is important to note that the average kinetic energy used here is limited to the translational kinetic energy of the molecules. That is, they are treated as point masses and no account is made of internal degrees of freedom such as molecular rotation and vibration. This distinction becomes quite important when you deal with subjects like the specific heats of gases. When you try to assess specific heat, you must account for all the energy possessed by the molecules, and the temperature as ordinarily measured does not account for molecular rotation and vibration. The kinetic temperature is the variable needed for subjects like heat transfer, because it is the translational kinetic energy which leads to energy transfer from a hot area (larger kinetic temperature, higher molecular speeds) to a cold area (lower molecular speeds) in direct collisional transfer.
KE = (3/2)kT, where k is the constant of proportionality.
Temperature is a measure of the average molecular kinetic energy of a substance. They are one and the same.
Vapor pressure is not rlated to the temp.
Molecular movement is directly related to temperature. As temperature increase, the additional energy is absorbed by the molecules. This energy is converted to motion energy and the molecules will move faster.
Kinetic energy is directly related to temperature, because temperature is the average kinetic energy of an object. Therefore, as the temperature of an object decreases, its kinetic energy decreases, as well.
Temperature is a measure of the average kinetic energy of the particles in an object. Temperatures also measure how kinetic energy is not how hot or cold it is. It's measuring what the amount of kinetic energy there when you throw something in the air and it comes back down.exampleThere is a ball on the top of a book shelf, and there is one on the bottom. Which one has more kinetic energy? The one on the top, because it has more time to fall and it has more kinetic energy.
solubility generally increases with a temperature increase
Temperature is the average kinetic energy of an object.
Its temperature.
we because is important
Temperature is the average kinetic energy of each individual particle inside an object.
Temperature
Matter is made up of particles (atoms and molecules); temperature is closely related to the average kinetic energy per particle. More precisely, the average kinetic energy per particle per degree of freedom.
No. The average kinetic energy of the individual particles in an object is basically related to the object's temperature.
if the temperature of the substance is raised then the kinetic energy of the gaseous particles will also increase....
Temperature is the average kinetic energy of each individual particle inside an object.
Temperature is a measure of the kinetic energy of the particles of a substance.
The term we use to describe this kind of measurement is "temperature". Note that temperature is not directly the average kinetic energy of the particles in an object (for one thing, temperature is measured in kelvins, kinetic energy is measured in joules). However, the two are related to each other.
Average kinetic energy on an atomic or molecular scale is what we perceive as temperature, and temperature is a major determinant of phase (along with pressure, which is the other major determinant).