(B) The average kinetic energy per molecule of an ideal gas is given by the formula: $E_k = \frac{3}{2}kT$. Here,$k$ is the Boltzmann constant $(1.38

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$6.17 \times 10^{-21} \text{ J}$

(B) The average kinetic energy per molecule of an ideal gas is given by the formula: $E_k = \frac{3}{2}kT$. Here,$k$ is the Boltzmann constant $(1.38 \times 10^{-23} \text{ J/K})$ and $T$ is the temperature in Kelvin. Given $T = 25\,^oC = 25 + 273 = 298 \text{ K}$. Substituting the values: $E_k = \frac{3}{2} \times 1.38 \times 10^{-23} \times 298 \approx 6.17 \times 10^{-21} \text{ J}$.

Class 11 Chemistry States of Matter Kinetic molecular theory of gases and Molecular collisions

Medium

The average kinetic energy of an ideal gas per molecule in $SI$ units at $25\,^oC$ will be

AIPMT 1996 All AIPMT

A
$6.17 \times 10^{-21} \text{ kJ}$
B
$6.17 \times 10^{-21} \text{ J}$
C
$6.17 \times 10^{-20} \text{ J}$
D
$6.17 \times 10^{-22} \text{ J}$

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States of Matter

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Kinetic molecular theory of gases and Molecular collisions

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