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Heat Transfer
Endo/Exothermic Processes
Energy Changes
Interpreting Graphs
Mixed Questions
100
A person with a body temperature of 37°C holds an ice cube with a temperature of 0°C. The direction of heat flow is
What is from the person's hand to the ice cube?
100

Fusion, or melting, is an endothermic process because energy is ____________

What is absorbed?

100

An open container of water is brought to a boil and heated until all of the water is converted to water vapor. Describe the changes in the water molecules.

What is molecules speed up and spread apart?

100
At what temperature does the triple point occur on the phase diagram?
What is 45-48 degrees Celsius?
100

Which substance listed is the best heat conductor and why? Copper, Aluminum, or silver? 

What is copper because it has a lower specific heat?

200
This is what happens to energy when water evaporates.
What is energy is absorbed into the system from the surroundings?
200

The energy-absorbing process by which a solid becomes a liquid is called

What is melting?

200

The diagram represents a phase change for some gold atoms. During this time, what happens to the kinetic energy of the atoms?

What is kinetic energy increases?

200
At what temperature would boiling occur at a pressure of 1 atm?
What is 60 degrees Celsius?
200

At what temperature is the freezing point of this substance?

What is -5 degrees Celsius?

300
This is what happens to thermal energy when gaseous water (vapor) condenses to liquid water.
What is energy is released from the system to the surroundings?
300

These phase changes are endothermic processes.

What are melting, vaporization, and sublimation?

300

The amount of energy needed to melt ice is the _____________________ as the amount needed to freeze water.

What is the same?

300
Between points X and Y, what phase(s) would be observed?
What is liquid and gas?
300

At what temperature is the boiling point of this substance?

What is 100 degrees Celsius?

400
How much heat in joules does it take to raise 10.0 g of water from 20.0°C to 40.0°C? [The specific heat of water is 4.18 J/g·°C]
What is 836 J?
400

These phase changes are exothermic processes.

What are freezing, condensation, and deposition.

400
Which points in the line represent an increase in kinetic energy?
What is A-B, C-D, E-F?
400
Describe the energy of the particles of the substance from point X to Y.
What is average kinetic energy (temperature) remains constant, and potential energy increases.
400

What term is defined as a measure of the average kinetic energy of the particles in a sample?

What is temperature?

500
Substance Specific Heat (J/g°C) Gold 0.13 Iron 0.46 Mercury 0.14 Silver 0.24 A 20.0 gram sample of an unknown substance was heated from 20 °C to 70 °C. The substance absorbed 240 Joules of heat energy in the heating process. Identify the substance.
What is .24 J/g°C?
500

This is what happens to kinetic energy when liquid water is heated.

What is kinetic energy increases?

500
Water cools from 32°C to 20°C. During this time, what happens to the kinetic energy of the molecules?
What is kinetic energy decreases?
500

Which numbered processes represent vaporization and freezing?

What are 1 & 4?

500

Draw a particle diagram showing the change from ice to water.

Ice particles should be closely packed together and liquid water particles should be loosely packed with space between particles.