Heat Calculations (bottom pgs 40+46 Energy Packet)

The temperature of a sample of water changes from 10. to 20. degrees Celsius when the water absorbs 420 Joules of heat energy. What is the mass of the sample?

• 1.0 g

• 10. g

• 100 g

• 1000 g

An 80.0 gram sample of water at 10.0 degress Celsius absorbs 1680 Joules of heat energy. What is the final temperature of the water?

• 50.0 degrees

• 15.0 degrees

• 5.00 degrees

• 4.00 degrees

The temperature of a sample of water changes from 10 to 20 degrees Celsius when the sample absorbs 418 Joules of heat energy, What is the mass of the sample?

• 1 g

• 10 g

• 100 g

• 1000g

A 36 gram sample of water has in initial temperature of 22 degrees Celsius. After the sample absorbs 1200 Joules of heat energy, the final temperature of the sample is . . .

• 8.0 degrees

• 14 degrees

• 30. degrees

• 55 degrees

When 200 grams of water cools from 50. to 25 degrees Celsius, the total amount of heat energy released by the water is . . .

• 42 kJ (42,000 J)

• 21 kJ (21,000 J)

• 34 J

• 17 J

What is the total number of Joules of heat energy absorbed by 15 grams of water when it is heated from 30. to 40. degrees Celsius?

• 42 J

• 63 J

• 130 J

• 630 J

What is the total amount of heat energy required to completely melt 347 grams of ice at its melting point temperature?

• 334 J

• 1,450 J

• 116,000 J

• 784,000 J

What is the amount of heat required to completely melt a 200. gram sample of H₂O at STP?

• 334 J

• 836 J

• 66,800 J

• 452,000 J

How much energy is required to vaporize 10.00 grams of water at its boiling point?

• 2.26 kJ (2260 J)

• 3.34 kJ (3340 J)

• 4.2 kJ (4200 J)

• 22.6 kJ (22,600 J)

What is the total number of kiloJoules required to boil 100. grams of water at 100 degrees Celsius and 1 atmosphere?

• 22.6 kJ (22,600 J)

• 33.4 kJ (33,400 J)

• 226 kJ (226,000 J)

• 334 kJ (334,000 J)