Specific Heat Review

What is the change in temperature when 50,000 Joules of energy is added to 200 grams of water at 25 C? The specific heat of water is 4.18 J/g°C

• 0.016 C
• 1,500 C
• 63 C
• 0.4 C

How many Joules of heat are required to change 10 gram of water from 20 C to 90 C? The specific heat of water is 4.18 J/g°C

• 1400 J
• 2800 J
• 210,000 J
• 1,400,000 J

3.4 g of aluminum foil was heated from 26 °C to 34 °C. How much heat was absorbed by the aluminum foil? (Specific heat of aluminum = 0.900 J/g °C)

• 24.48 J

• 0.47 J

• 2.16 J

• 79.56 J

If a 18 g ring has a temperature rise of 20.5°C, 1296 J of energy are released. Calculate the specific heat capacity of the ring.

• 1.13 J/g °C

• 0.0006 J/g °C

• 3.51 J/g °C

The temperature of a sample of water increases from 25°C to 54°C as it absorbs 5,672 J of heat. What is the mass of the sample? The specific heat of water is 4.18 J/g°C

• 25.1 g

• 46.7 g

• 54.3 g

How much heat is released when 32 g of water at 98°C cools to 10°C? The specific heat of water is 4.18 J/g°C

• 11,770 J

• 0.086 J

• 0.66 J

• 13,153 J

37 g of copper was heated from 26°C to 52°C. How much energy was used to heat Cu? (Specific heat capacity of Cu is 0.385 J/g °C)

• 268.78 J

• 370.37 J

• 3.69 J

The temperature of a sample of 20.2 g of iron changed from 72.5 °C to 59.8 °C with the release of 115.44 J of heat. What is the specific heat of iron?

• 0.45 J/g °C

• 0.62 J/g °C

• 0.80 J/g °C

A 113 g sample of an unknown substance was heated from 22.5°C to 53°C. In the process, the substance absorbed 2378.42 J of energy. What is the specific heat of the substance?

• 0.69 J/g °C

• 0.97 J/g °C

• 0.45 J/g °C

How much heat is needed to raise a 789 g piece of aluminum from 34°C to 65°C? (Specific heat of aluminum = 0.900 J/g•°C)

• 20, 451 J

• 22,013 J

• 19,149 J