Understanding Energy and Heat Concepts

Define energy and distinguish between kinetic and potential energy.

• Energy is the ability to do work; kinetic energy is energy due to motion, while potential energy is stored energy.

• Energy is the ability to do work; kinetic energy is stored energy, while potential energy is energy due to motion.

• Energy is the ability to do work; both kinetic and potential energy are forms of thermal energy.

• Energy is the ability to do work; kinetic energy is energy due to temperature, while potential energy is energy due to pressure.

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NGSS.MS-PS3-4

NGSS.MS-PS3-5

Explain how energy changes accompany chemical reactions.

• Energy is always absorbed in chemical reactions.

• Energy is always released in chemical reactions.

• Energy can be either absorbed or released during chemical reactions, depending on the nature of the reaction.

• Energy remains constant during chemical reactions.

Tags

NGSS.HS-PS1-4

Describe the relationship between heat, thermal energy, and temperature.

• Heat is the same as thermal energy, and temperature is a measure of both.

• Heat is the transfer of thermal energy, and temperature is a measure of the average kinetic energy of particles.

• Thermal energy is the same as temperature, and heat is a measure of both.

• Temperature is the transfer of heat, and thermal energy is a measure of temperature.

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NGSS.MS-PS3-4

NGSS.MS-PS1-4

Calculate the amount of heat required to raise the temperature of 100 g of water from 20°C to 80°C. (Specific heat of water = 4.18 J/g°C)

• 25,080 J

• 41,800 J

• 16,720 J

• 20,900 J

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NGSS.MS-PS3-4

Define specific heat and heat capacity.

• Specific heat is the amount of heat required to change the temperature of a unit mass of a substance by 1°C; heat capacity is the total amount of heat required to change the temperature of a substance by 1°C.

• Specific heat is the total amount of heat required to change the temperature of a substance by 1°C; heat capacity is the amount of heat required to change the temperature of a unit mass of a substance by 1°C.

• Specific heat and heat capacity are the same and refer to the amount of heat required to change the temperature of a substance.

• Specific heat is the amount of heat required to change the temperature of a substance by 1°C; heat capacity is the amount of heat required to change the temperature of a unit mass of a substance by 1°C.

Tags

NGSS.HS-PS3-4

A metal block with a mass of 2 kg has a specific heat of 0.5 J/g°C. How much heat is needed to increase its temperature by 10°C?

• 10,000 J

• 1,000 J

• 100 J

• 5,000 J

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NGSS.MS-PS3-4

Differentiate between chemical and physical changes in terms of energy changes.

• Chemical changes involve energy changes, while physical changes do not.

• Both chemical and physical changes involve energy changes, but chemical changes often involve larger energy changes.

• Physical changes involve energy changes, while chemical changes do not.

• Neither chemical nor physical changes involve energy changes.

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NGSS.MS-PS3-4

NGSS.MS-PS3-5

What is the formula to calculate the heat absorbed or released by a substance?

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NGSS.MS-PS3-4

NGSS.MS-PS3-5

A 500 g sample of a substance requires 2,000 J of heat to increase its temperature by 5°C. What is the specific heat of the substance?

• 0.8 J/g°C

• 0.4 J/g°C

• 1.6 J/g°C

• 0.2 J/g°C

Explain the physical implications of a high specific heat capacity.

• A substance with a high specific heat capacity heats up and cools down quickly.

• A substance with a high specific heat capacity requires more heat to change its temperature, thus heats up and cools down slowly.

• A substance with a high specific heat capacity does not change temperature.

• A substance with a high specific heat capacity changes temperature rapidly with little heat.

Tags

NGSS.MS-PS3-4