Sentences with phrase «average kinetic»

Heating occurs when the average kinetic energy of the molecules in the thing rises.

Temperature is a measurement of average kinetic energy.

Within each region of the atmosphere that contains CO2, and within each region of the Earth surface, some molecules have above average kinetic energy and some have below average kinetic energy; the temps of the regions are proportional to the means of the kinetic energies in those regions, but the molecules are not all the same.

From jim2's link: «It is important to note that the average kinetic energy used here is limited to the translational kinetic energy of the molecules.

If two bodies have the same average kinetic energy of their atoms, the will have the same temperature no matter how large [i.e. how much mass] the bodies are.

The rate at which water molecules in the skin layer escape to the atmosphere is determined by their average kinetic energy, ie their temperature.

The TEMPERATURE of the water (its average kinetic energy) determines the rate of both evaporation and radiation.

The average kinetic energy of the skin layer — not one single flux contributing to that energy — determines its temperature (and emission and evaporation).

I haven't a clue why you have served me up this garbled explanation — «kinetic energy aka heat», «average kinetic energy, aka temperature», «The energy flow through the atmosphere hasn't changed one bit, but radiative energy has been converted to kinetic energy.

Water molecules in a liquid have a temperature (average kinetic energy) and a Boltzmann distribution of energies.

Increased DLR does NOT directly eject water molecules into the air, it must FIRST raise the temperature (average kinetic energy) of the skin layer.

That's because the average kinetic energy just is 3 / 2kT, where k is the Boltzmann constant.

The average kinetic energy of a number of molecules is not independent of height.

That molecules speeding past a kilometer high o n the moon has an average kinetic energy independent of the height?

The average kinetic energy at any height is inversely related to the potential energy.

That is, the average kinetic energy of molecules at height z, plus its potential energy at that level, is a conserved quantity?

«The average kinetic energy of a set of molecules [as they] freely fly to higher heights is independent of that height»

Question Of those molecules that fly one kilometer high or higher, what is their average kinetic energy as they pass through a height of one kilometer?

Answer The average kinetic energy of the molecules that freely fly to any given height is independent of that height.

No, temperature is a measure of the average kinetic energy of the molecules of a substance, radiatively active or not.

A mercury thermometer is going to register the same reading for a highly radiative gas like CO2 as it is for a barely radiative gas like N2 when they have the same average kinetic energy in the molecules.

That's not a gravito - thermal effect, since all speed distributions (and hence average kinetic energies) are independent of height.

A measure of the average kinetic energy of the particles in a sample of matter, expressed in terms of units or degrees designated on a standard scale.

For small numbers of molecules, temperature is no longer strictly proportional to the average kinetic energy.

Molecules of one mass don't have the same average kinetic energy as more massive or less massive molecules.

DeWitt Payne: «If the particles do not obey MB statistics, and they probably won't for small numbers, the justification for converting average kinetic energy to temperature using MB statistics (2/3 KE / k) no longer exists.»

He appears to think it's fine that molecules in the upper shell have more total energy, on average, than molecules in the lower shell so long as average kinetic energy is the same.

In which case the temperature (as measured by its average kinetic energy as it passes through a given level) is independent of height.

Temperature is related directly to the average kinetic energy of the molecules in the gas.

In equilibrium, molecules of one mass have the same average kinetic energy as molecules of a different mass.

If the particles do not obey MB statistics, and they probably won't for small numbers, the justification for converting average kinetic energy to temperature using MB statistics (2/3 KE / k) no longer exists.

What's stated is that eventually the average kinetic energy (the temperature) of all molecules will be the same throughout the gas.

If those two containers have the same temperature, they have the same average kinetic energy per particle (for a monatomic gas).

(a) Energy conservation implies that every molecule loses kinetic energy as it travels upward, so that the average kinetic energy of all molecules decreases with height.

The first was one where the gas in a box, in Earth's gravity, have different temperatures (average kinetic energies) at the top of the box and at the bottom of the box.

That temperature is proportional to average kinetic energy per particle in the canonic limit is a secondary derivation from this primary thermodynamic concept.

Heat is energy, temperature is average kinetic motion, which is one - type - of energy.

You only get a lapse rate if you assume that temperature is always strictly proportional to average kinetic energy.

For a small number of particles in the control volume, temperature is no longer strictly proportional to the average kinetic energy.

Average kinetic energy of the entire system means little, as that will not change unless energy is removed from the system or inputted to the system.

As implausible as it might seem at first, the average kinetic energy of the molecules that make it 17 km will be the same as the average KE of the molecules at the bottom.

Over a sufficiently long period of time, it follows from the equipartition theorem and other principles of statistical mechanics that every molecule in a gas will have the same average kinetic energy, the same average potential energy, and the same total energy, as any other molecule.

He said we indeed can measure the average kinetic energy.

It looks to me like it comes from a belief that all the molecules in a volume have exactly the average kinetic energy, overlooking the variation.

This in turn makes it hard to verify the soundness of its reasoning; at one point it incorporated the virial theorem that average potential energy is twice average kinetic energy, which however doesn't apply at all to the atmosphere because the frequency of molecular collisions is many orders of magnitude too high for the theorem to hold.

(The temperature of air depends on the average kinetic energy of its molecules.)

Temperature is a measure of the average kinetic energy of the random motions of the particles, or atoms that make up a material.

Also, as the faster - moving molecules escape, the remaining molecules have lower average kinetic energy, and the temperature of the liquid thus decreases.

The answer is that temperature is a measure of the average kinetic energy of the gas atoms, that is, a measure of how fast they are moving.

Not exact matches

Then they used the speed of sound measurement to calculate the average speed of the argon molecules and hence the average amount of kinetic energy that they had — from this they were able to calculate the Boltzmann constant with an extremely high accuracy.