Heat of Fusion, Heat of Vaporization, and Specific Heat

When water is heated from 10°C to 15°C What is the change in temperature?

• 10 °C
• 5 °C
• 15 °C
• 25 °C

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

How much energy is required to heat up 12000 g of copper from 10 °C to 120 °C. The specific heat capacity is 0.390 J/g°C.

• 46800 J

• 561600 J

• 514800 J

Tags

NGSS.HS-PS3-1

How many Joules of energy are required to make 100 grams of ice at 0 ^οC completely melt? The specific latent heat of fusion of ice is 334 J/g

• 200 J

• 400 J

• 33,400 J

• 2,000,000 J

Tags

NGSS.HS-PS3-1

The heat absorbed by melting a solid is known as

• latent heat of fusion

• latent heat of solid

• latent heat of liquid

• latent heat of vaporisation

Tags

NGSS.HS-PS3-2

Water molecules have the greatest kinetic energy in

• Ice at 0 ⁰C

• Water at 90 ⁰C

• Water at 373 K

• Steam at 150 ⁰C

Tags

NGSS.HS-PS3-2

The amount of energy required to raise the temperature 1ºC for every gram is called____?

• Thermal Energy

• Specific Heat

• Temperature

• Kinetic Energy

How much energy is needed to raise the temperature of 5.0 grams of lead from 25°C to 35°C? [specific heat (c) = 0.129 J/(g•°C)]

• 6.45 J/(g•°C)

• 6.45 J

• 16.1 J/(g•°C)

• d.16.1 J

Tags

NGSS.HS-PS3-1

Which of the following best explains why the sand at the beach is hotter than the water?

• Sand has a higher specific heat than water.

• Sand has a lower specific heat than water.

• There is more water than sand at the beach.

• There is more sand than water at the beach.

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

• 12.82 °C
• 24.12°C
• 351 °C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

Consider the following temperature-time graph when a solid is heated. which part of the graph involves latent heat of vaporization?

• Part I

• Part II

• Part III

• Part IV

Tags

NGSS.MS-PS1-4