No. There is a well known distribution of probabilities that describes how likely it is that a given molecule has a given kinetic energy, but a gas will always have some fast and some cold molecule. The average KE is defined by temp, however.
NO - the molecules in a sample of gas are expected to have a Maxwell-Boltzman distribution of velocities. There is a finite probability for molecules to have any particular speed, from zero to near-lightspeed, but the probabilities of those speeds are described by the Maxwell-Boltzman distribution. As the internal energy of the gas increases, the mean velocity increases. In theory all the molecules could have that same mean velocity, but the probability is so incredibly small that even for a very small gas sample you would never expect to observe such a phenomena during the life of the universe.
NO. Depending on there molecular weight it should vary. Heavier gases should have more kinetic energy. But i will like to have second opinion. ( Galileo's experiment of small and big balls falling from height. )
As the temperature increases, the kinetic energy of the molecules will increase. As the temperature decreases, the kinetic energy of the molecules will decrease.
False
The average kinetic energy of a gas is directly proportional to its temperature. This is described by the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly related to the temperature of the gas. As temperature increases, the average kinetic energy of the gas molecules also increases.
The average kinetic energy of the gas molecules increases. This is because temperature is directly proportional to kinetic energy, as stated by the Kinetic Theory of Gases. Therefore, as the temperature increases, the molecules have higher kinetic energy.
This statement is correct according to the kinetic theory of gases. The average kinetic energy of gas molecules is directly proportional to the temperature of the gas. This means that at a given temperature, all gas molecules will have the same average kinetic energy.
temperature. This is known as the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly proportional to the temperature of the gas, regardless of the type of gas.
Yes, two gases at the same temperature have the same average kinetic energy. Temperature is a measure of the average kinetic energy of the particles in a substance. Therefore, if two gases are at the same temperature, their particles have the same average kinetic energy.
The average kinetic energy of a gas is directly proportional to its temperature. This is described by the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly related to the temperature of the gas. As temperature increases, the average kinetic energy of the gas molecules also increases.
The average kinetic energy of the gas molecules increases. This is because temperature is directly proportional to kinetic energy, as stated by the Kinetic Theory of Gases. Therefore, as the temperature increases, the molecules have higher kinetic energy.
This statement is correct according to the kinetic theory of gases. The average kinetic energy of gas molecules is directly proportional to the temperature of the gas. This means that at a given temperature, all gas molecules will have the same average kinetic energy.
Yes. because expansion depends upon kinetic energy of the molecules and at same temperature the molecules of both the gases have the same average kinetic energy.
temperature. This is known as the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly proportional to the temperature of the gas, regardless of the type of gas.
Yes, two gases at the same temperature have the same average kinetic energy. Temperature is a measure of the average kinetic energy of the particles in a substance. Therefore, if two gases are at the same temperature, their particles have the same average kinetic energy.
Pressure is the effect of collisions with molecules. KMT -- molecules have kinetic energy due to their temperature which imparts more velocity, hence kinetic energy, to the molecules. All gases have KE due to temperature. IF absolute zero was ever achieved there would be no kinetic energy in the molecules, no molecular motion, no collisions, no pressure.
Heat energy in a substance is the intensity of vibration of the molecules in that substance. The more the vibration more is the heat energy stored in the object. So in a way Heat energy is the kinetic energy of the molecules in the substance. Thus temperature increases on the increase in the kinetic energy of the gases.
In gases their kinetic energy rises
All gases have same kinetic energy of molecules at same conditions.
The kinetic energy of gases varies depending on factors such as temperature and pressure. In general, gases have higher kinetic energy at higher temperatures due to increased molecular motion. The average kinetic energy of gas molecules can be calculated using the formula KE = (1/2)mv^2, where m is the mass of the molecule and v is its velocity.
The kinetic energy is lowest in solids, higher in liquids, and highest in gases.