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Average Kinetic Energy Equation:
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The average kinetic energy per molecule in an ideal gas is given by the equation KE_avg = (3/2)kT, where k is Boltzmann's constant and T is the absolute temperature in Kelvin. This fundamental relationship connects temperature directly to molecular motion.
The calculator uses the average kinetic energy equation:
Where:
Explanation: This equation shows that the average kinetic energy of gas molecules is directly proportional to the absolute temperature, with Boltzmann's constant serving as the proportionality factor.
Details: Calculating average kinetic energy is essential for understanding gas behavior, thermodynamics, and molecular dynamics. It provides insight into temperature at the molecular level and is fundamental to kinetic theory of gases.
Tips: Enter temperature in Kelvin. The Boltzmann constant is fixed at its standard value of 1.380649 × 10⁻²³ J/K. Temperature must be greater than 0 K.
Q1: Why is the factor 3/2 used in the equation?
A: The factor 3/2 comes from the three translational degrees of freedom in three-dimensional space, with each degree contributing (1/2)kT to the energy.
Q2: What is Boltzmann's constant?
A: Boltzmann's constant (k) is a fundamental physical constant that relates the average kinetic energy of particles in a gas with the temperature of the gas.
Q3: Can this equation be used for all gases?
A: This equation applies specifically to ideal monatomic gases. For diatomic and polyatomic gases, additional factors for rotational and vibrational energies must be considered.
Q4: Why must temperature be in Kelvin?
A: The Kelvin scale is an absolute temperature scale where 0 K represents absolute zero, making it appropriate for thermodynamic calculations involving molecular motion.
Q5: How does kinetic energy relate to temperature?
A: Temperature is a measure of the average kinetic energy of the particles in a substance. Higher temperature means greater average kinetic energy of the molecules.