Procedure Part 1 – Cooling a Metal Cube in Water In this part of…
Procedure Part 1 – Cooling a Metal Cube in Water In this part of…
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Procedure
Part 1 – Cooling a Metal Cube in Water
In this part of the lab, we measured the differences in final temperature of a series of known metal cubes.
that are cooled in water.
1. Construct the following table.
| Metal | Trial # | mass of metal (g) | Initial Temp. Metal (°C) |
Mass Solution (g) |
initial Temp. Solution (°C) |
Final Temp. Metal/Solution (°C) |
| Copper | trial 1 | 72.73 g | 81°C | 42.78g | 22°C | 27.6°C |
| Aluminum | trial 2 | 22.15g | 95°C | 51.4g | 22°C | 25.4°C |
| Iron | trial 3 | 60.71 | 92°C | 45.84g | 21°C | 28.6°C |
Part 2 – Specific Heat Capacity of an Unknown Metal
In part 2 you we identified an unknown metal solid by measuring the specific heat capacity indirectly in a
calorimetry experiment.
1. Construct the following table.
| Trial # | Mass Metal (g) |
Initial Temp. Metal (°C) |
Mass water (g) | Initial Temp. Water (°C) |
Final Temp. Metal/Water (°C) |
| trial 1 | 56.86g | 99°C | 68.53g | 22°C | 25°C |
| trial 2 | 56.86g | 98°C | 75.65g | 22°C | 24.7°C |
| trial 3 | 56.86g | 98°C | 76.21g | 22°C | 24.4°C |
Part 3 -Specific Heat Capacity of 1.0M NaCl
In this part of the lab, we measured the specific heat capacity of 1.0M NaCl solution.
1. Construct the following table.
| Trial # | Identity of Metal |
Initial Temp. Metal (°C) | Mass water (g) | Initial temp water (°C) | Final Temp. Metal/Solution (°C) |
| trial 1 | copper | 97°C | 46.59.g | 24°C | 34.9°C |
| trial 2 | aluminum | 97°C | 46.59g | 24°C | 27°C |
| trial 3 | iron | 97°C | 46.59g | 24°C | 40.8°C |
Specific Heat Capacity – Worksheet
1. Define specific heat capacity. Consider the units of the variable when.
writing your definition.
2. Calculate the delta T of the room temperature water for each metal cube trial in part 1. If all the
volumes of the metal cubes are essentially the same, what variable(s) account for the different
changes in temperature of the water? Explain and discuss using your experimental data.
3. Consider the specific heat capacities of the metals used in part 1 tabled below. For which
metal is the most heat (in J) stored per gram of material? Explain.
| Metal | Literature cmetal (J/g°C) |
| copper | 0.384 |
| aluminum | 0.897 |
| Iron | 0.447 |
4. Calculate the final temperature of the water, Tf, expected if a 75.0 g copper metal cube at
95.0 °C is added to 50.00 g of water at 20.0 °C.
5. Calculate the specific heat of the unknown metal in part 2 (use Eqn 5 from the procedure).
Determine an average value for the three trials.
6. Identify the unknown metal based on the specific heat.
Metal Literature cmetal (J/g°C)
| Metal | Literature cmetal (J/g°C) |
| Brass | 0.402 |
| aluminum | 0.897 |
| Iron | 0.447 |
| steel | 0.502 |
| copper | 0.384 |
7. Calculate a % error in your average specific heat.
8. Suggest two sources of error from your measurement in part 2 and how that would impact
your specific heat.
9. Calculate the specific heat capacity of your prepared 1.0 M HCl solution. Determine an
average value for the three trials.
10. Based on your data, is it reasonable to assume the specific heat capacity of a 1.0M salt
solution is the same as pure water?
References
- 9.2 Calorimetry – Chemistry: Atoms First 2e | OpenStax, accessed Oct. 2022.
- https://openstax.org/books/chemistry-atoms-first-2e/pages/9-2-calorimetry
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