6.2 Thermal Energy Review

Only the cup itself

The cup, the water inside, and the air inside the cup

Only the lid and the cup walls

Only the surrounding room air

A colorful logo printed on the cup

A lid and double walls that reduce matter and energy transfer

A wider opening to allow more air in

A thin single wall that quickly equalizes temperature

They cannot keep liquids hot.

They are also able to keep liquids hot.

They only work with metal cups.

They require ice to function.

It increases evaporation and speeds matter loss.

It helps maintain temperature and slows matter loss from the system.

It allows more gas to enter and exit the system.

It cools the liquid immediately by adding air.

Particles in gases have a lot of space between them; particles in liquids do not.

Particles in liquids have more space than particles in gases.

Particles in solids have more space than particles in gases.

Particles in gases and solids have the same spacing.

Temperature cannot change in closed systems.

Light, heat, or cold may interact with the system and cause a temperature change.

Only evaporation can change temperature.

Only adding more liquid can change temperature.

It is absorbed, warming the matter it shines on.

It disappears without affecting temperature.

It cools the liquid by removing energy.

It turns into particles of matter.

It increases due to energy transfer.

It also decreases equally.

It stays constant because systems are isolated.

It fluctuates randomly without pattern.

Particles in colder water move more and have higher kinetic energy.

Particles in hotter water move more and have higher kinetic energy.

Particle speed is unrelated to kinetic energy.

Particles in gases move less than in liquids when hot.

Energy moves from cooler to warmer matter, increasing the cooler sample’s temperature.

Energy transfers from warmer to cooler matter, changing temperatures over time.

No energy transfers because they are separate samples.

Energy moves only if the samples are both solids.