Calorimetry Principles and Applications
A Grade 12 Chemistry worksheet exploring the principles, types, and applications of calorimetry, including calculations and experimental design.
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Calorimetry Principles and Applications
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Read each question carefully and provide thorough answers. Show all calculations where applicable.
1. Which of the following best describes the primary function of a calorimeter?
To measure the rate of a chemical reaction.
To determine the heat capacity of a substance.
To measure the change in enthalpy of a chemical or physical process.
To analyze the elemental composition of a sample.
2. In a bomb calorimeter, why is the reaction vessel sealed and immersed in a known quantity of water?
To prevent evaporation of the sample.
To ensure the reaction occurs at constant pressure.
To measure the heat transferred to or from the surroundings.
To maintain a constant volume for the reaction.
3. A calorimeter is an apparatus used to measure the amount of evolved or absorbed during a chemical or physical change.
4. The specific heat capacity of a substance is the amount of required to raise the temperature of one gram of the substance by one degree Celsius.
5. Describe the key differences between a bomb calorimeter and a coffee-cup calorimeter, highlighting their respective applications and limitations.
6. Observe the diagram of a typical coffee-cup calorimeter below. Identify the labeled components and explain the function of each in the calorimetry experiment.
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B:
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7. A 5.00 g sample of an unknown metal at 90.0 °C is placed into a coffee-cup calorimeter containing 50.0 g of water at 22.0 °C. The final temperature of the water and metal is 25.3 °C. Assuming no heat loss to the surroundings and the specific heat capacity of water is 4.18 J/g°C, calculate the specific heat capacity of the unknown metal.
8. A perfect calorimeter would completely prevent any heat exchange with the surroundings.
True
False