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As stated in the kinetic-molecular theory, the temperature of a substance is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles.
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Equation is one important result of the kinetic theory: The average molecular kinetic energy is proportional to the ideal gas law's absolute temperature. From equations ( 1 ) and ( 3 ), we have P V = 2 3 K t . {\displaystyle PV={\frac {2}{3}}K_{t}.}
The 2/3 factor in the proportionality reflects the fact that velocity components in each of the three directions contributes ½ kT to the kinetic energy of the particle. The average translational kinetic energy is directly proportional to temperature: \[\epsilon = \dfrac{3
kinetic energy, form of energy that an object or a particle has by reason of its motion. If work, which transfers energy, is done on an object by applying a net force, the object speeds up and thereby gains kinetic energy. Kinetic energy is a property of a moving.
The average kinetic energy for a mole of particles, KE avg, is then equal to: KE avg = 1 2 M u rms 2 KE avg = 1 2 M u rms 2 where M is the molar mass expressed in units of kg/mol.
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