Question

1. a student says gases cannot be compressed because \particles dont shrink.\ which statement correctly addresses this misconception?

a. the claim is correct because gas particles cannot change size.
b. the claim is incorrect because gas particles move into smaller orbits.
c. the claim is correct because compression reduces kinetic energy.
d. the claim is incorrect because particles are far apart and can be pushed closer.

1. a student says real gases behave like ideal gases when they have strong attractions. which statement correctly evaluates this claim?

a. the claim is correct because strong attractions prevent collisions.
b. the claim is correct because real gases have small volumes.
c. the claim is incorrect because ideal gases are assumed to have no attractions.
d. the claim is incorrect because ideal gases form chemical bonds easily.

1. a gas is cooled at constant volume. a student claims \pressure stays the same because particle number stays the same.\ which correction is accurate?

a. pressure decreases because collisions with the container become less frequent.
b. pressure increases because particles move farther apart.
c. pressure stays the same because energy cannot change in a closed system.
d. pressure increases because particles slow down.

1. a student says boyle’s law means \pressure and volume go up together.\ which statement correctly explains the relationship?

a. the claim is correct because it is a direct relationship.
b. the claim is incorrect because pressure and volume are inversely related.
c. the claim is correct because temperature changes.
d. the claim is incorrect because pressure depends only on particle size.

1. a student says thomson discovered the nucleus. which statement correctly evaluates this claim?

a. the claim is correct because thomson discovered protons.
b. the claim is incorrect because thomson only discovered electrons.
c. the claim is correct because the plum pudding model includes a nucleus.
d. the claim is incorrect because electrons are found in the nucleus.

1. a student claims that the bohr model is the modern model. which statement is correct?

a. the bohr model uses orbits, but the modern model uses orbitals based on probability.
b. the bohr model describes electrons as stationary.
c. the modern model has no energy levels.
d. the bohr model places electrons inside the nucleus.

1. a student looks at rutherford’s gold foil data and says: \since most particles passed through are solid.\

a. the claim is correct because the nucleus blocks most particles.
b. the claim is incorrect because atoms are mostly empty space.
c. the claim is correct because electrons absorb alpha particles.
d. the claim is incorrect because the nucleus has no charge.

Explanation:

Question 12

To address the misconception about gas compression:

• Option A: Gas particles can't change size, but gases can be compressed (particles are far apart and can be pushed closer), so A is wrong.
• Option B: Compression doesn't reduce kinetic energy; it increases pressure due to more frequent collisions, so B is wrong.
• Option C: The claim is wrong (gases can be compressed), so C is wrong.
• Option D: Gases can be compressed because particles are far apart and can be pushed closer, so the claim is incorrect, and D is correct.

For real vs ideal gases:

• Ideal gas assumption: no intermolecular attractions. Real gases behave like ideal gases when intermolecular attractions are weak (low pressure, high temperature).
• Option A: Strong attractions don't prevent collisions; ideal gas has no attractions, so A is wrong.
• Option B: Real gases have particle volume, but ideal gas assumes negligible volume; strong attractions mean real gas is less like ideal, so B is wrong.
• Option C: Ideal gases are assumed to have no attractions, so real gases with strong attractions don't behave like ideal gases (claim is incorrect), so C is correct.
• Option D: Ideal gases don't form chemical bonds, so D is wrong.

Gas cooled at constant volume (Gay - Lussac's Law: \(P\propto T\) at constant \(V\)):

• When cooled, temperature (\(T\)) decreases, so kinetic energy of particles decreases. Particles move slower, so collisions with container are less frequent, pressure (\(P\)) decreases.
• Option A: Matches the above reasoning, correct.
• Option B: At constant volume, particles can't move farther apart; pressure should decrease, so B is wrong.
• Option C: Energy can change (heat is removed), and pressure changes, so C is wrong.
• Option D: Slower particles lead to less frequent collisions, lower pressure, so D is wrong.

Answer:

D. The claim is incorrect because particles are far apart and can be pushed closer.

Question 13