Question

1. which statement of molecules of the gas is in accord with the kinetic molecular theory?

a. the gas molecules have attractive forces between them.
b. the gas molecules are in constant, random motion.
c. the gas molecules are relatively large and have significant volume.
d. the gas molecules have collisions without transferring energy.

1. according to the kinetic theory of gases, which description is correct?

a. energy may be transferred between colliding particles.
b. the volume of gas molecules prevents random motion.
c. a gas particle is fixed in its position.
d. gas particles are strongly attracted to each other.

1. which of these statements of the kinetic molecular theory is/are not true for real gases with low temperatures or high pressures?

i. gas molecules only interact with each other momentarily, i.e., through collisions.
ii. the volume of gas is entirely empty by mostly space; these molecules of gas are negligible.
iii. collisions between gas molecules are elastic, negligible energy is lost in these collisions.
a. i only
b. i and ii only

Explanation:

Question 12 (Assuming the first question is about gas particles and kinetic molecular theory)

To determine the correct statement about gas particles according to the kinetic molecular theory, we analyze each option:

• Option A: Gas particles do not have attractive forces between them (a key postulate of the kinetic molecular theory), so this is incorrect.
• Option B: Gas particles are in constant, random motion, which is a fundamental postulate of the kinetic molecular theory. This is correct.
• Option C: Gas particles are not stationary; they are in constant motion, so this is incorrect.
• Option D: Gas particles do not lose energy in elastic collisions (another postulate), so this is incorrect.

Analyzing each option based on the kinetic theory of gases:

• Option A: Energy can be transferred between colliding particles (in elastic collisions, kinetic energy is conserved but can be transferred between particles), so this is correct.
• Option B: The volume of gas particles is negligible compared to the volume of the container, not that it prevents motion, so this is incorrect.
• Option C: Gas particles move in random paths, not fixed paths, so this is incorrect.
• Option D: Gas particles do not lose energy in elastic collisions, so this is incorrect.

• Statement I: In real gases, molecules do interact (have attractive/repulsive forces), so "only interact with each other measurably, i.e., strongly" is not accurate for all real gas situations, but at low temp/high pressure, intermolecular forces become significant. However, the first part "Gas molecules..." (assuming the full statement is about real gas behavior) – actually, in real gases, intermolecular forces exist, so if Statement I is about real gas molecules having interactions, but the wording here is a bit off. Wait, let's re - evaluate:
• Statement II: The volumes of gas molecules are not negligible at high pressure (since the gas is compressed, the volume of the molecules themselves becomes a significant portion of the total volume), so "The volumes of gas molecules are entirely negligible" is incorrect for real gases at high pressure/low temp.
• Statement III: Collisions between gas molecules are elastic (a postulate of ideal gases, but real gases have inelastic collisions due to intermolecular forces? No, actually, the kinetic molecular theory for ideal gases assumes elastic collisions, but real gases have intermolecular forces, but collisions between molecules are still mostly elastic, but the main deviations for real gases at low temp/high pressure are intermolecular forces and molecular volume. Wait, maybe the question is about which postulates of the ideal gas kinetic theory do not hold for real gases at low temp/high pressure.

Ideal gas postulates: 1. Gas particles have negligible volume. 2. No intermolecular forces. 3. Elastic collisions.
For real gases at low temp/high pressure:

• Molecular volume is not negligible (so postulate 1 fails) – related to Statement II (if Statement II is "The volumes of gas molecules are entirely negligible" – this is a postulate that fails for real gases at high pressure, so Statement II is a postulate that doesn't hold.
• Intermolecular forces are significant (so postulate 2 fails) – related to Statement I (if Statement I is about gas molecules only interacting measurably, i.e., strongly – but actually, in real gases, intermolecular forces exist, so if the ideal gas postulate is no intermolecular forces, then Statement I is about the real gas behavior (molecules do interact), but the question is which postulates (of ideal gas) do not hold.
• Collisions: Ideal gas has elastic collisions, real gas collisions are still mostly elastic, so postulate 3 holds.

Wait, maybe the options are about the postulates that are violated for real gases at low temp/high pressure.
If Statement I: "Gas molecules only interact with each other measurably, i.e., strongly" – no, in real gases, intermolecular forces exist but not always "strongly" in all cases, but at low temp/high pressure, they become significant. But the ideal gas postulate is no intermolecular forces, so the violation is that intermolecular forces exist (so Statement I is about the real gas having interactions, which is a violation of the ideal gas postulate of no intermolecular forces).
Statement II: "The volumes of gas molecules are entirely negligible" – this is an ideal gas postulate, and for real gases at high pressure, molecular volume is not negligible, so this postulate is violated.
Statement III: "Collisions between gas molecules are elastic, supplying energy to each other" – ideal gas postulate is elastic collisions (kinetic energy is conserved, not that they "supply energy" in a non - conserved way). Wait, elastic collisions mean kinetic energy is conserved, so if Statement III is saying that collisions supply energy (implying a…

Answer:

B. The gas particles are in constant, random motion.

Question 13 (About kinetic theory of gases)