Definition
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Definition

What is a catalyst and how does it work?

By definition, a catalyst is not consumed or used up. The nature of a catalytic reaction is often defined as: “A substance, usually present in small amounts related to the reactants, that modifies and especially increases the rate of a chemical reaction without being consumed in the process.”

How do they work?

Normally smoke will burn or oxidize, at a temperature of 540C (1,000F) or higher. Burning a stove this hot would require continuous intense fire and would require a higher wood consumption. The answer to eliminate this is the catalytic combustor.

Wood smoke gases coming in contact with the catalyst, causes chemical changes to take place. This will then allow the smoke to ignite at temperatures around 260C (500F). This temperature is easily achieved in the firebox of a woodburning stove. As the wood gases ignite and burn within the catalytic combustor, clean by-products of water vapor (H20) and carbon dioxide (CO2) are emitted.

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