Chemistry 101 Assignment 3

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Apr 3, 2024

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Chemistry Lab Report Title: Determination of the Heat Capacity of a Metal Date: March 23, 2024 Objective: To determine the heat capacity of a metal sample using the method of calorimetry. Materials: 100 mL beaker Metal sample (unknown) Thermometer Water Bunsen burner Stopwatch Balance Procedure: Measure the mass of the metal sample using the balance. Place the metal sample in the 100 mL beaker. Add a known volume of water to the beaker. Measure the initial temperature of the water. Heat the beaker with the metal sample and water using the Bunsen burner. Stir the mixture and continue heating until the temperature reaches a steady state. Record the final temperature of the water. Calculate the heat capacity of the metal using the formula: Q=mcΔTQ=mcΔT, where QQ is the heat gained or lost, mm is the mass of water, cc is the specific heat capacity of water, and ΔTΔT is the change
in temperature. Data: Mass of metal sample: 25.0 g Initial temperature of water: 25.0°C Final temperature of water: 35.0°C Mass of water: 150.0 g Specific heat capacity of water (cc): 4.18 J/g°C Observations: The metal sample appeared to be a shiny, silver-colored solid. The temperature of the water increased steadily as heat was applied. Calculations: Q=mcΔTQ=mcΔT Q=(150.0g)(4.18J/g°C)(35.0°C − 25.0°C)Q=(150.0g)(4.18J/g°C)(35.0°C − 25.0°C) Q=6270JQ=6270J Results: The heat gained by the water is calculated to be 6270 J. Since the heat lost by the metal is equal to the heat gained by the water (by the principle of conservation of energy), the heat capacity of the metal can be determined. Discussion: The calculated heat capacity of the metal sample will be discussed here, along with any discrepancies or sources of error observed during the experiment.
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