At the same temperature and pressure, which of the following gases will have highest kinetic energy per molecule (at. wt. of hydrogen = 1, nitrogen = 14, carbon = 12, oxygen = 16)?

Question

At the same temperature and pressure, which of the following gases will have highest kinetic energy per molecule (at. wt. of hydrogen = 1, nitrogen = 14, carbon = 12, oxygen = 16)? (A) Hydrogen gas (B) Nitrogen gas (C) Ethylene gas (D) All will have equal-average kinetic energy

Tardigrade Admin · Accepted Answer

Average kinetic energy per molecule (= (3/2) k T) does not depend upon the molar mass. At a given temperature, all the gases would have equal average kinetic energy.

Q. At the same temperature and pressure, which of the following gases will have highest kinetic energy per molecule (at. wt. of hydrogen = 1, nitrogen = 14, carbon = 12, oxygen = 16)?

Hydrogen gas

Nitrogen gas

Ethylene gas

All will have equal-average kinetic energy

Average kinetic energy per molecule $(= \frac{3}{2} k T)$ does not depend upon the molar mass. At a given temperature, all the gases would have equal average kinetic energy.

Q. At the same temperature and pressure, which of the following gases will have highest kinetic energy per molecule (at. wt. of hydrogen = 1, nitrogen = 14, carbon = 12, oxygen = 16)?

Hydrogen gas

Nitrogen gas

Ethylene gas

All will have equal-average kinetic energy

Average kinetic energy per molecule (=23​kT) does not depend upon the molar mass. At a given temperature, all the gases would have equal average kinetic energy.

Average kinetic energy per molecule $(= \frac{3}{2} k T)$ does not depend upon the molar mass. At a given temperature, all the gases would have equal average kinetic energy.