Kinetic molecular theory of gases and Molecular collisions Questions in English

(B) According to the kinetic theory of gases, the average speed of gas molecules is proportional to $\sqrt{T}$. Since the frequency of collisions is directly proportional to the average speed of the molecules, it follows that the frequency of collisions increases in proportion to the square root of temperature $(\sqrt{T})$.

(C) The average kinetic energy of gas molecules is given by the formula $KE_{avg} = \frac{3}{2} k_B T$, where $k_B$ is the Boltzmann constant and $T$ is the absolute temperature.
Since $k_B$ is a constant, the average kinetic energy is directly proportional to the absolute temperature $T$.

(C) $1$. An ideal gas is a theoretical model that obeys gas laws under all conditions of temperature and pressure.
$2$. The kinetic molecular theory assumes that ideal gas molecules have no volume and no intermolecular forces of attraction.
$3$. Since these conditions cannot be met by real gases, an ideal gas does not exist in reality.