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Chemistry of Hand Warmers

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by

Matthew Hodgkins

on 10 June 2015

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Transcript of Chemistry of Hand Warmers

Combines with air to make rust and heat to have your fingers or toes stay warm.
MICROPOROUS POUCH
The little bag that the solution is inside so you can have more air react with the solution. lets air in but then it can't be released.
Activated Charcoal
Helping add heat evenly through the hands and keeps from burning skin. How do you activate this? You open the package of the hand warmers and shake them till they get hot it's as simple as that.
Iron Powder
Chemical structure
This is sodium acetate trihydrate
Chemical equation
4Fe(s)+302(g)-> 2Fe203(s)


The heat given off by an air activated Hand warmer is caused by a chemical reaction . The iron within the hand warmer mixes with the oxygen in the air and oxides, because it gives off heat when it reacts the process is known as an exothermic oxidation.

How is chemistry involved?
Chemistry of Hand Warmers
Whats it's made of?
SODIUM CHLORIDE
Chemistry's Role

THANKS FOR WATCHING
We eat about 2 million pounds of iron powder each year in our favorite (fortified) breakfast cereals. Yum!
Fun Facts
Like in your kitchen, salt amplifies things. As a de-icer in snowy cities, salt can cause car underbellies to corrode. Here too NaCl (with an assist from H2O) is a handy catalyst that kicks the rust reaction into gear.
A pound of activated charcoal has the same surface area as six football fields—that's a lot of crannies for storing water.
Vermiculus
Latin word. Hydrated magnesium aluminum silicate looks like worms as it expands The result is a light, highly absorbent, chemically inert, odorless, and fire-resistant super material. Along with the activated charcoal, it helps diffuse the iron powder so the filings don't burn too quickly (and don't burn your skin)
Endothermic vs Exothermic
This is an exothermic reaction beause it gives heat off.
Full transcript