6T6_ Posted April 13, 2018 Share Posted April 13, 2018 I’m a noob when it comes to things chemistry. Is the burning point of sodium metal (s) and H20 (l) enough to melt through certain objects? Like a door of wood. Since capillary action doesn’t happen with metals that don’t absorb.... could a design using spit amounts of water on top of raw sodium metal to form a sort of blowtorch. I’m not sure when oxidation comes into play with the metals.... can someone explain? Link to comment Share on other sites More sharing options...
StringJunky Posted April 13, 2018 Share Posted April 13, 2018 1 hour ago, 6T6_ said: I’m a noob when it comes to things chemistry. Is the burning point of sodium metal (s) and H20 (l) enough to melt through certain objects? Like a door of wood. Since capillary action doesn’t happen with metals that don’t absorb.... could a design using spit amounts of water on top of raw sodium metal to form a sort of blowtorch. I’m not sure when oxidation comes into play with the metals.... can someone explain? I think the water will carry the heat away as it's heated. Link to comment Share on other sites More sharing options...
6T6_ Posted April 14, 2018 Author Share Posted April 14, 2018 4 hours ago, StringJunky said: I think the water will carry the heat away as it's heated. Using minuscule amount of it as a reactant to prevent a go to completion so that some of the sodium remains...wouldn’t that work then as it would reheat the remaining sodium oxide. H2O(l) + Na2O(s) yields(heated) H2O(l) + Na2O(s) through a double displacement reaction right? If I were to use amount of it to superheat the sodium or a surrounding conducting metal, wouldn’t that work? The fact that water evaporate though would pose problems so another compound of 1+ or 1- valence would be used. Link to comment Share on other sites More sharing options...
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