Lemon battery: Difference between revisions
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Revert deletions by Apau98. If numbers are wrong, don't badmouth them, correct them. (Debunking of widespread myth that "one lemon can light a flashlight bulb") |
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[[Image:Lemon battery.svg|thumb|right|A '''lemon cell''' battery is made with a lemon and two metallic [[electrodes]] of different metals such as a copper penny or a copper plating and a galvanized (zinc coated) nail.]] |
[[Image:Lemon battery.svg|thumb|right|A '''lemon cell''' battery is made with a lemon and two metallic [[electrodes]] of different metals such as a copper penny or a copper plating and a galvanized (zinc coated) nail. In practice, a single lemon cell is incapable of lighting a light bulb or even a flashlight bulb. It would take over 9000 lemons to power a flashlight bulb. See [[Lemon_battery#Calculations|Calculations]]. ]] |
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A '''lemon battery''' is a device used in [[experiments]] proposed in many science textbooks around the world.<ref>[http://www.hilaroad.com/camp/projects/lemon/lemon_battery.html Lemon Battery<!-- Bot generated title -->]</ref> It is made by inserting two different [[metal]]lic objects, for example a [[galvanization|galvanized]] [[nail (engineering)|nail]] and a [[copper]] coin, into a [[lemon]]. The copper coin serves as the positive electrode or cathode and the galvanized nail as the electron-producing negative electrode or anode. These two objects work as [[electrode]]s, causing an [[electrochemistry|electrochemical]] reaction which generates a small [[potential difference]]. |
A '''lemon battery''' is a device used in [[experiments]] proposed in many science textbooks around the world.<ref>[http://www.hilaroad.com/camp/projects/lemon/lemon_battery.html Lemon Battery<!-- Bot generated title -->]</ref> It is made by inserting two different [[metal]]lic objects, for example a [[galvanization|galvanized]] [[nail (engineering)|nail]] and a [[copper]] coin, into a [[lemon]]. The copper coin serves as the positive electrode or cathode and the galvanized nail as the electron-producing negative electrode or anode. These two objects work as [[electrode]]s, causing an [[electrochemistry|electrochemical]] reaction which generates a small [[potential difference]]. |
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In current practice, zinc is produced by [[electrowinning]] of [[zinc sulfate]] or pyrometallurgic reduction of zinc with carbon. The energy produced originates from this source. |
In current practice, zinc is produced by [[electrowinning]] of [[zinc sulfate]] or pyrometallurgic reduction of zinc with carbon. The energy produced originates from this source. |
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== Calculations == |
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1 lemon can generate approximately 0.83 Volts. The reaction typically ranges from 0.80V - 0.98V |
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[[Volts]] x [[Amperes]] = [[Watt]]s |
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1 lemon = 0.83V x 0.00015 Amps = 0.0001245 Watts |
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Flashlight bulb = 2.4V x 0.5 Amps = 1.2 Watts, or 9,639 lemons |
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Halogen bulb = 12V x 0.83 Amps = 10 Watts, or 80,321 lemons |
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LED bulb = 2.8V x 0.0006 Amps = 0.000498 Watts,or four lemons |
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== Reactions == |
== Reactions == |
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Revision as of 02:29, 22 January 2011
A lemon battery is a device used in experiments proposed in many science textbooks around the world.[1] It is made by inserting two different metallic objects, for example a galvanized nail and a copper coin, into a lemon. The copper coin serves as the positive electrode or cathode and the galvanized nail as the electron-producing negative electrode or anode. These two objects work as electrodes, causing an electrochemical reaction which generates a small potential difference.
Overview
The aim of this experiment is to show students how batteries work. After the battery is assembled, a multimeter can be used to check the generated voltage. In order for a more visible effect to be produced, a few lemon cells connected in series can be used to power a standard LED. Flashlight bulbs are generally not used because the lemon battery cannot produce the amount of current required to light such bulbs. Digital clocks can work well, and some toymakers offer small kits with a clock that can be powered by two potatoes or lemons.
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4 Lemon Circuit (How to video: <ref>http://www.youtube.com/watch?v=AY9qcDCFeVI Create a Lemon Battery -
Diagram
Energy source
The energy for the battery does not come from the lemon or potato, but rather the energy comes from the chemical change in the zinc (or other metal). The zinc is oxidized inside the lemon, exchanging some of its electrons in order to reach a lower energy state, and the energy released provides the power. The lemon or potato merely provides an environment where this can happen, but they are not used up in the process.
In current practice, zinc is produced by electrowinning of zinc sulfate or pyrometallurgic reduction of zinc with carbon. The energy produced originates from this source.
Calculations
1 lemon can generate approximately 0.83 Volts. The reaction typically ranges from 0.80V - 0.98V
1 lemon = 0.83V x 0.00015 Amps = 0.0001245 Watts
Flashlight bulb = 2.4V x 0.5 Amps = 1.2 Watts, or 9,639 lemons
Halogen bulb = 12V x 0.83 Amps = 10 Watts, or 80,321 lemons
LED bulb = 2.8V x 0.0006 Amps = 0.000498 Watts,or four lemons
Reactions
In a lemon battery, both oxidation and reduction occur. Consider the case of a zinc-copper battery; this battery is similar to the original "simple voltaic cells" invented by Alessandro Volta.[2] At the anode, metallic zinc is oxidised, and enters the acidic solution as Zn2+ ions:
- Zn → Zn2+ + 2 e-.
At the copper cathode, hydrogen ions (solvated protons from the acidic solution) are reduced to form molecular hydrogen:
- 2H++ 2e- → H2.
Variations
Potatoes,[3] apples, or any other fruit or vegetable containing acid or other electrolyte can be used, but lemons are preferred because of their higher acidity.[4] In potatoes, for instance, the electrolyte is phosphoric acid, while in lemons it is citric acid. Other non-rusty metal combinations (such as magnesium-copper) are more effective; for example, using a magnesium strip instead of zinc increases the voltage from 1.1 V with zinc to 1.6 V with magnesium. (The exact voltage varies depending on the lemons.) However, zinc and copper are usually preferred because they are reasonably safe and easy to obtain.
See also
References
- ^ Lemon Battery
- ^ Oon, Hock Leong (2007). Chemistry Expression: An Inquiry Approach. Panpac Education Pte Ltd. p. 236. ISBN 9789812711625.
- ^ Potato Battery
- ^ Food Batteries