Calorimetry Principles and Applications
A Grade 12 Chemistry worksheet on calorimetry, covering specific heat capacity, heat transfer calculations, and experimental applications.
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Calorimetry Principles and Applications
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Read each question carefully and provide your answers in the space provided. Show all your work for calculations.
1. Define calorimetry and explain its primary purpose in chemistry.
2. The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius is called its .
3. In an isolated system, the total energy remains constant; therefore, the heat lost by one component is to the heat gained by another component.
4. Which of the following statements is true regarding a bomb calorimeter?
It measures heat changes at constant pressure.
It measures heat changes at constant volume.
It is used for reactions involving aqueous solutions.
It is typically used to determine the specific heat capacity of a substance.
5. A 25.0 g sample of an unknown metal at 98.0 °C is placed in a coffee-cup calorimeter containing 50.0 g of water at 22.0 °C. The final temperature of the water and metal is 28.5 °C. Assuming no heat loss to the surroundings and a specific heat capacity of water of 4.18 J/g°C, calculate the specific heat capacity of the metal.
6. In an exothermic reaction, heat is absorbed from the surroundings, causing the temperature of the surroundings to decrease.
True
False
7. Label the parts of the calorimeter shown in the diagram below.
A.
B.
C.
D.