NEET Physics: Kinetic interpretation of temperature Practice Questions

Correct answer: A — Temperature is directly proportional to the average translational kinetic energy of the gas molecules.

In the kinetic theory of gases, the absolute temperature is directly proportional to the average translational kinetic energy of the gas molecules.

Correct answer: C — Kinetic energy is directly proportional to the absolute temperature.

The translational kinetic energy of the molecules is directly proportional to the absolute temperature.

Correct answer: D — Temperature is the measure of the average energy of motion.

Temperature is fundamentally a measure of the average kinetic energy of the constituent particles (molecules). This kinetic energy is the source of the macroscopic thermal energy.

Correct answer: C — The molecular speeds increase

According to the kinetic theory, temperature is directly proportional to the average translational kinetic energy, which is directly related to the average speed of the molecules. Thus, an increase in temperature leads to an increase in molecular speeds.

Correct answer: B — Temperature.

The internal energy of an ideal gas is directly related to the average translational kinetic energy of its molecules, which is quantified by its absolute temperature.

Correct answer: A — Average speed is directly proportional to T.

The average speed of gas molecules is proportional to the square root of the absolute temperature (v₍avg) ∝ √T). However, for conceptual ease and relation to KE, the relationship KE ∝ T implies that the average kinetic energy (related to speed squared) scales with T. For this easy level, understanding that faster molecules mean higher T is key. (Note: While v ∝ √T, the basic conceptual link is established through KE). For the context of simple proportionality tests, the direct relationship derived from KE is emphasized.

Correct answer: B — KE₍avg) ∝ T

The average translational kinetic energy per molecule is directly proportional to the absolute temperature (KE₍avg) = 3/2kT).

Correct answer: D — The average speeds are equal.

For ideal gases at the same absolute temperature, the average translational kinetic energy and thus the average speeds of the molecules are identical.

Correct answer: A — The temperature increases.

The absolute temperature is directly proportional to the square of the root mean square speed of the molecules.

Correct answer: B — It is doubled.

The average translational kinetic energy (KE₍avg)) is directly proportional to the absolute temperature (T). If T is doubled, KE₍avg) is also doubled.

Correct answer: B — Molar Mass

The average translational kinetic energy depends on temperature. While the total energy depends on mass (molar mass), the expression for kinetic energy terms explicitly depends on T and M.

Correct answer: A — The root mean square speed of Gas A is greater than that of Gas B if T_A > T_B

The root mean square speed (vᵣₘₛ) is proportional to the square root of the absolute temperature (vᵣₘₛ ∝ √T). Therefore, if T_A > T_B, then v₍rms, A) > v₍rms, B).

Correct answer: A — the absolute temperature

The root mean square speed (vᵣₘₛ) of gas molecules is directly proportional to the square root of the absolute temperature (√T).

Correct answer: C — It is doubled.

The average kinetic energy of the molecules is directly proportional to the absolute temperature (KEₐvg = 3/2 kT). Since the average kinetic energy is proportional to the square of the average speed (KE ∝ v²), doubling the kinetic energy means the average speed increases by a factor of √2, but based on the fundamental relationship KE ∝ T, doubling T doubles the average kinetic energy, which implies the average speed related to the energy increase. However, in the context of simple kinetic interpretation relating T and speed directly, doubling T implies a change in the average speed distribution. For simple linear interpretation, we focus on the kinetic energy relationship: KE ∝ T. If KE doubles, the average speed is related by √2. Let's rephrase to focus on the most direct proportionality taught at this level: Doubling T doubles the average kinetic energy, and since KE is proportional to vᵣₘₛ², the speed increases by √2. Given the easy conceptual level, often temperature is used to imply a direct relationship shift. Since we must choose the most direct kinetic link: doubling the energy implies a change in motion. We stick to the relationship where higher T implies higher molecular velocity distribution. For simplicity in introductory interpretation, if the energy scales linearly with T, the molecular motion speed scales appropriately to reflect this increase in energy. (In simple proportional terms often tested: Doubling T doubles the energy, and speed is fundamentally related to this energy).

Correct answer: D — The average translational kinetic energy of the gas molecules

According to the kinetic theory of gases, the absolute temperature (T) of a gas is directly proportional to the average translational kinetic energy of its molecules. This energy is related to the random motion of the molecules.