4 ms·

> 2 Sn2+ → Sn4+ + Sn This isn’t a redox reaction though. Those are tin ions in equilibrium with each other.. so no combustion. > I'll ask the chemists in the

> 2 Sn2+ → Sn4+ + Sn This isn’t a redox reaction though. Those are tin ions in equilibrium with each other.. so no combustion. > I'll ask the chemists in the house if they know of any such reactions tomorrow since Google isn't being much use I’d be interested what you find out, my chemistry knowledge has aged… theres always stuff I don’t know! Edit: Yep you’re correct it is considered a redox, but not combustion.

gpm 5y ago
> This isn’t a redox reaction though. Those are tin ions in equilibrium with each other.. so no combustion. I agree I wouldn't call this example combustion (which is typically required to be highly exothermic and therefore not easily reversible), but I believe it is a redox reaction. It's the transfer of electrons from one ion to another, which meets the definition I was taught. Wikipedia seems to agree, both with my definition of redox reaction [1], and that this is one [2]. [1] https://en.wikipedia.org/wiki/Redox https://en.wikipedia.org/wiki/Redox [2] (See Introduction and History): https://en.wikipedia.org/wiki/Disproportionation https://en.wikipedia.org/wiki/Disproportionation
deleted 5y ago
[deleted]
gpm 5y ago
> I’d be interested what you find out So they (two chemistry PhD students) both agree that it should be possible, but don't have any great examples. They point at disproponation as the right class of reactions (where I got Sn2+ from). They agree that the different ends of a hydrocarbon can react in a redox reaction, but at least for common chemicals it's usually a slow reaction. For more combustion like examples what I got was "maybe look at peroxides" and "maybe caro's acid" (H2SO5). I can't find anyone who actually managed to get Caro's acid outside of aqueous solution to explode it (in a reaction not involving water)... so I can't find anyone who is stating authoritatively what would happen if you managed to do so. I can find plenty of explosive peroxides in literature, but haven't found any that are a simple redox reaction... Anyways, I'm reasonably satisfied that it should in some sense be possible, even if not practical.

gpm 5y ago

> This isn’t a redox reaction though. Those are tin ions in equilibrium with each other.. so no combustion. I agree I wouldn't call this example combustion (which is typically required to be highly exothermic and therefore not easily reversible), but I believe it is a redox reaction. It's the transfer of electrons from one ion to another, which meets the definition I was taught. Wikipedia seems to agree, both with my definition of redox reaction [1], and that this is one [2]. [1] https://en.wikipedia.org/wiki/Redox https://en.wikipedia.org/wiki/Redox [2] (See Introduction and History): https://en.wikipedia.org/wiki/Disproportionation https://en.wikipedia.org/wiki/Disproportionation

deleted 5y ago

[deleted]

gpm 5y ago

> I’d be interested what you find out So they (two chemistry PhD students) both agree that it should be possible, but don't have any great examples. They point at disproponation as the right class of reactions (where I got Sn2+ from). They agree that the different ends of a hydrocarbon can react in a redox reaction, but at least for common chemicals it's usually a slow reaction. For more combustion like examples what I got was "maybe look at peroxides" and "maybe caro's acid" (H2SO5). I can't find anyone who actually managed to get Caro's acid outside of aqueous solution to explode it (in a reaction not involving water)... so I can't find anyone who is stating authoritatively what would happen if you managed to do so. I can find plenty of explosive peroxides in literature, but haven't found any that are a simple redox reaction... Anyways, I'm reasonably satisfied that it should in some sense be possible, even if not practical.