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Use aluminum foil, salt water, and activated charcoal to construct a simple battery strong enough to power a small motor or light.
Clip one end of each electrical lead to each terminal of the electrical device. Clip the other end of one of the leads to the aluminum foil. Firmly press the final clip on the pile of charcoal, then watch what happens.
If the battery doesn’t seem to be working after a few seconds, you may need to reduce its internal resistance. Try increasing the contact area between the clip and the charcoal by folding the entire battery over the clip—like a taco—and pressing down hard. Make sure that the clip stays buried in the charcoal. If you are using a motor, you can also try kickstarting it by briefly spinning the flag.
Batteries convert chemical energy into electrical energy. They have two electrodes—called a cathode and an anode—where chemical reactions that either use or produce electrons take place. The electrodes are connected by a solution—called an electrolyte—through which ions can move, completing an electrical circuit. In this activity, the salt provides ions that can move through the wet paper towel and transfer charge.
To generate electrical energy, this battery relies on oxidation of aluminum at the anode, which releases electrons, and a reduction of oxygen at the cathode, which uses electrons. The movement of electrons through an external circuit generates an electric current that can be used to power simple devices. A diagram of the battery and equations for the half and overall reactions are given below:
Equations for the half and overall reactions:
anode: Al(s) + 3OH−(aq) → Al(OH)3(s) + 3e−
cathode: O2(g) + 2H2O(l) + 4e− → 4OH−(aq)
overall: 4Al(s) + 3O2(g) + 6H2O(l) → 4Al(OH)3(s)
Aluminum foil provides an affordable supply of aluminum. Activated charcoal, which is mostly made of carbon, can conduct electricity and is non-reactive. It provides a highly porous surface that is exposed to oxygen in the air. One gram of activated charcoal can have more internal surface area than an entire basketball court! This surface provides a large number of sites to which oxygen can bind and participate in the cathode reaction.
This large reaction area makes it possible for the simple aluminum–air battery to generate 1 volt (1 V) and 100 milliamps (100 mA). This is enough power to run a small electrical device and provides a safe and easy way to make a powerful battery at home or in school.
The first modern electric battery was made up of a series of electrochemical cells, called a voltaic pile. To make a voltaic pile, repeat Assembly steps 1–4 to construct additional aluminum–air cells. Stack two or three aluminum–air cells on top of each other to see if you can make a more powerful battery. Clip one lead to the bottom piece of foil and place the other lead in the top charcoal pile. Press down firmly on the pile to reduce the internal resistance of the battery, but make sure that the foil pieces don’t touch each other. If the foil from one cell is in contact with the foil from the cell above it, the electrons will bypass the paper towel and activated charcoal and move directly into the second piece of foil, which has a lower resistance than the charcoal layer. This effectively shorts out the lower cell, which no longer contributes to the overall power output.
You can compare the power qualitatively by looking at the intensity of the electrical device or quantitatively by taking measurements on a multimeter. Use a multimeter to measure the voltage and current generated by your battery. What changes to the battery design result in a larger voltage or current?
Calculate the power output from your battery by calculating the product of its voltage and current. Try to power other devices that require higher voltage or current, such as a string of LEDs (make sure they’re connected in the right orientation), a piezo buzzer, or a more powerful light.
Small electrical devices are available at electronic stores. Make sure the chosen electrical device will produce a noticeable change when connected to a one-volt power supply.
This activity demonstrates oxidation and reduction reactions—integral parts of battery chemistry. The use of atmospheric oxygen as the oxidizing agent has extensions to other redox reactions that occur in corrosion, metabolism, and combustion. In addition, the participation of oxygen as a reactant in the aluminum–air battery can be used to introduce the concepts of fuel cells and alternative energy sources.
This activity is based on a demonstration by teachers from the Galileo Workshop in Japan.
Use your skin and different metals to create a battery.
Light an LED with five cents.
Make a conductivity meter and let your electrolytes shine.
This work is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License.
Attribution: Exploratorium Teacher Institute