The average kinetic energy of an ideal gas per molecule in si unit at 25 degree celsius is
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Answered by
184
Well the answer of your question is " 6.2 * 10^-21 J "
Actually the average kinetic energy can easily be determined by the formula :
3/2 KT . Here K is the boltzmann constant which is equal to 1.38x10^-23 J/K
and T representing the temperature in kelvin
25 degree celsius = 298 kelvin so by just putting the values in the formual
Average kinetic energy = 3/2 × 1.38x10^-23 × 298 = 6.2 * 10^-21 J
So the answer will be 6.2 * 10^-21 J
Actually the average kinetic energy can easily be determined by the formula :
3/2 KT . Here K is the boltzmann constant which is equal to 1.38x10^-23 J/K
and T representing the temperature in kelvin
25 degree celsius = 298 kelvin so by just putting the values in the formual
Average kinetic energy = 3/2 × 1.38x10^-23 × 298 = 6.2 * 10^-21 J
So the answer will be 6.2 * 10^-21 J
Answered by
88
The average kinetic energy of an ideal gas can be calculated using the formula - (3/2) kT, where k is known as Boltzmann's constant and T is the ideal gas's absolute temperature measured in Kelvins.
Since it is given as per molecule, then it can be calculated using the formula - 3/2 NₐkbT, where Nₐ is the Avogadro number.
So, Kavg (Average Kinetic energy) per molecule = 3/2 NₐkbT
= 3/2 x 8.314/6.022 x (10)⁻²³ x 298
= 6.17 x 10⁻²¹ kJ K-1
Since it is given as per molecule, then it can be calculated using the formula - 3/2 NₐkbT, where Nₐ is the Avogadro number.
So, Kavg (Average Kinetic energy) per molecule = 3/2 NₐkbT
= 3/2 x 8.314/6.022 x (10)⁻²³ x 298
= 6.17 x 10⁻²¹ kJ K-1
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