Lesson 8.4 MC Practice - Phase Change Calculations

What is the total amount of heat absorbed by 100.0 grams of water when the temperature of the water is increased from 30.0῾°C to 45 °C?

• 418 J

• 6,270 J

• 12, 500 J

• 18,800 j

Tags

NGSS.HS-PS3-4

The temperature of a sample of water changes from 10°C to 20°C when the sample absorbs 418 joules of heat What is the mass of the sample?

• 1g

• 10 g

• 100 g

• 1000 g

A 36. gram sample of water has an initial temperature of 22 °C. After the sample absorbs 1200 joules of heat energy, the final temperature of the sample is

• 8.0 °C

• 14 °C

• 30 °C

• 55 °C

Tags

NGSS.HS-PS3-4

How many Joules of heat energy are released when 50. grams of water are cooled from 70 °C to 60 °C?

• 42 J

• 210 J

• 2,100 J

• 4200 J

Tags

NGSS.HS-PS3-4

NGSS.HS-PS3-1

The temperature of 100. grams of water changes from 16.0 °C to 20.0 °C. What is the total number of Joules of heat energy absorbed by the water?

• 105

• 168

• 420.

• 1680

Tags

NGSS.HS-PS3-4

When 420. Joules of heat energy is added to 10. grams of water at 20.°C, the final temperature of the water will be

• 10°C

• 30°C

• 40 °C

• 100 °C

Tags

NGSS.HS-PS3-4

What is the total amount of heat required to completely vaporize 347 grams of liquid water at its boiling point?

• 334 J

• 1,450 J

• 116,000 J

• 784,000 J

Tags

NGSS.HS-PS3-1

The heat energy required to change a unit mass of a liquid into a gas at constant temperature is called

• heat of vaporization

• heat of formation

• heat of solution

• heat of fusion

What is the minimum amount of heat required to completely melt 20.0 grams of ice at its melting point?

• 20.0 J

• 83.6 J

• 6,680 J

• 45,200 J

Tags

NGSS.HS-PS3-1

The heat energy required to change a unit mass of a solid into a liquid at constant temperature is called

• heat of vaporization

• heat of formation

• heat of solution

• heat of fusion