# Dramatic Demonstration of Thermal Conductivity and Specific Heat Capacity Mark as Favorite (46 Favorites)

DEMONSTRATION in Heat, Specific Heat, Temperature, Unlocked Resources. Last updated October 30, 2019.

### Summary

In this demonstration, students will observe the high thermal conductivity and low heat capacity of copper metal.

High School

### NGSS Alignment

This demonstration will help prepare your students to meet the performance expectations in the following standards:

• HS-PS3-1: Create a computational model to calculate the change in the energy of one component in a system when the change in energy of the other component(s) and energy flows in and out of the system are known.
• Scientific and Engineering Practices:
• Constructing Explanations and Designing Solutions
• Engaging in Argument from Evidence

### Objectives

By the end of this demonstration, students should be able to

• understand the difference between thermal conductivity and specific heat capacity

### Chemistry Topics

This demonstration supports students’ understanding of

• Specific Heat Capacity
• Thermal Conductivity
• Properties of Matter
• Energy transfer

### Time

Teacher Preparation: 10 minutes

Lesson: 20 minutes

### Materials

• 20 g of coiled copper wire
• 400-mL or 600-mL beaker
• Tap water
• Hot plate
• Thermometer or temperature probe
• Tongs

### Safety

• Students should wear proper safety gear during chemistry demonstrations. Safety goggles and lab apron are required.
• Exercise caution when using a heat source. Hot plates should be turned off and unplugged as soon as they are no longer needed.
• If there are water droplets on the copper wire when you remove it from the boiling water, the water will burn!!
• Do not allow students to perform this experiment.

### Teacher Notes

• A video of the demonstration can be found in the download box at the top of the page.
• Heat is an artifact of the transfer of energy. For thermal energy transfer, molecules must come into contact with each other. The transfer of energy occurs continuously on a particulate/molecular level. On the macroscopic scale, however, we will notice that “Thermal Equilibrium” is reached when the temperatures of the objects are equal.
• Copper has an exceptionally high thermal conductivity, but a very low specific heat capacity.
• Thermal conductivity is a measure of how well a substance conducts heat. The higher the thermal conductivity, the greater the rate of heat transfer. Since copper has very high thermal conductivity it will release heat quickly.
• Specific heat capacity if a measure of how much heat is needed to raise the temperature of a substance. Typically, it is the amount of heat (joules) required to raise the temperature of one gram of a substance by one degree (°C). Since copper has very low specific heat capacity it requires very little energy to raise its temperature.
• Copper will change temperature very quickly when it is removed from the water. Some of the energy is lost to the air in the transfer AND when the copper touches your hand, the energy needed to lower the temperature of the copper is very low, due to its low specific heat capacity. Meaning, that not much energy is transferred to your hand, and risk of burning your hand is very low.