Specific Heat
Chemistry Name
Q = m C ∆T
1. ____________________ is the amount of energy that it takes to raise the temperature of 1 gram of a substance by 1 K
2. ____________________ is the temperature at which all molecular motion ceases
3. ____________________ process is a change in matter in which energy is absorbed
4. ____________________ process is a change in matter in which energy is released
5. What is the specific heat of a substance that absorbs 2500 joules of heat when a sample of 100 g of the substance
increases in temperature from 10 °C to 70°C?
6. If 200 grams of water is to be heated from 24.0°C to 100.0°C to make a cup of tea, how much heat must be added?
The specific heat of water is 4.18 J/g∙C
7. How many grams of water would require 2200 joules of heat to raise its temperature from 34°C to 100°C? The
specific heat of water is 4.18 J/g∙C
8. A block of aluminum weighing 140 g is cooled from 98.4°C to 62.2°C with the release of 1080 joules of heat. From
this data, calculate the specific heat of aluminum. Check your answer with a specific heat table.
9. 100.0 mL of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4.18 J/g°C, calculate
the amount of heat energy needed to cause this rise in temperature.
10. A total of 54.0 joules of heat are absorbed as 58.3 g of lead is heated from 12.0°C to 42.0°C. From these data, what is
the specific heat of lead?
