What is the activation energy for a match?

AI Thread Summary
The discussion centers on the use of nichrome wire and high voltage to ignite matches, sparked by a YouTube video demonstration. The analysis involves calculating the wattage produced by nichrome wire at various voltages, emphasizing that prolonged connection to a power source can yield significant energy transfer. A key point of inquiry is the energy required to ignite a match, which remains unspecified in available resources. The composition of matches is highlighted, noting that potassium chlorate (KClO3) serves as the oxidizer, decomposing at 400 degrees Celsius, while phosphorus sesquisulfide (P4S3) has a flash point around 100 degrees Celsius. The combustion process is detailed, describing the decomposition of P4S3 into phosphorus and sulfur dioxide, followed by complex oxidation reactions that can produce phosphoric and sulfuric acids in the presence of water.
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I saw a YouTube video where someone took nichrome wire and a high voltage source and managed to light a whole series of matches.

I got me curious so I ran some numbers on how much wattage could be produced for a given length of nichrome wire and a given voltage. And assuming time is no issues you could leave said power source connected to the wire for as long as possible and in theory get a very high amount of joules of energy transfer, but exactly how much energy is required to ignite a match, couldn't find anything online anywhere with specific numbers.
 
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Most matches are made with potassium chlorate KClO3 as oxidizer and phosphorus sesquisulfide P4S3.
2 KClO3 decomposes to 2 KCl and 3 O2, at 400 degrees C.
Phosphorus sesquisulfide has a flash point around 100 degrees C, so once the oxidation starts, the P4S3 acts as the main fuel for the match. I think it decomposes to P4 and 3 SO2. P4, in turn, oxidizes to P4O10 in a complex, multi-step reaction. SO2 oxidizes to form SO3.
Then, if there is water in the atmosphere, P4O10 + 6 H2O -> 4 H3PO4 (–177 kJ) making phosphoric acid. Also, SO3 + H2O -> H2SO4 (-88 kJ), making sulfuric acid.
 

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