Thermodynamics Review

Why can’t all of the energy in a system be used to do work?

• Energy is destroyed during a process

• Entropy causes some energy to become unavailable

• All energy is used for heat

• Energy is always constant and never changes

Tags

NGSS.HS-PS3-4

Why does water heat heat up and cool down VERY SLOWLY?

• High Specific Heat

• Low Specific Heat

• It's solid

• It's always cold

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NGSS.HS-PS3-4

Entropy increases from solid, liquid to gas. Why?

• Molecular disorder increases

• Molecules increase in number from solid to gas

• Molecules are heavier in solid

• Molecules are more reactive

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NGSS.MS-PS1-4

Given the change of phase: CO₂(g) —> CO₂(s). As CO₂(g) changes to CO₂(s), the entropy of the system

• decreases

• increases

• remains the same

Which represents a decrease in entropy?

• sublimation of CO₂

• boiling water

• condensation of steam on cold glass

• NaCl dissolving in water

Identify whether the following result in an increase or decrease in entropy:

3 moles of gas (on reactant side) --> 6 moles of gas (product)

• increase

• decrease

There is a natural tendency for energy to spread out.

• True

• False

Tags

NGSS.HS-PS3-4

For a process to be 100% efficient, which of the following would need to happen regarding entropy?

• Entropy must increase

• Entropy must remain constant

• Entropy must decrease

• Entropy must be zero

Ice is absorbing heat over time. The image shows its temperature as time passes. Which parts of the graph represent an increase in internal potential energy and a phase change? Select all that apply.

• 1

• 2

• 3

• 4

• 5

Tags

NGSS.HS-PS3-2

NGSS.HS-PS3-4

If object A and B have the same temperature, and object C is the same temperature as object A the all three are the same temperature. This tendency illustrates which of the following laws of thermodynamics?

• Zeroth Law

• First Law

• Second Law

• Third Law