The helium and argon are put in the flask at the same room temperature (300 K). The ratio of average kinetic energies (per molecule) of helium and argon is :
❓ Question The helium and argon gases are placed in a flask at the same room temperature (300 K) . What is the ratio of their average kinetic energies (per molecule) ? 🖼️ Question Image ✍️ Short Solution Step 1 — Recall the formula for average kinetic energy per molecule For any gas, according to the kinetic theory of gases , the average kinetic energy of a molecule is: E k ‾ = 3 2 k T where k k = Boltzmann constant (1.38 × 10⁻²³ J/K) T T = absolute temperature in kelvin Step 2 — Dependence on temperature Notice that the average kinetic energy per molecule depends only on temperature , not on the nature (mass or type) of the gas. That means — if two gases are at the same temperature, each molecule has the same average kinetic energy regardless of whether the gas is light (like helium) or heavy (like argon). Step 3 — Apply given data Given: T He = T Ar = 300 K T_{\text{He}} = T_{\text{Ar}} = 300~\text{K} So, E He = 3 2 k T He...