2 mhchem

As far as I know thermite is a typical redox reaction where $$Al + Fe^{3+} \rightarrow Fe + Al^{3+}$$$$\ce{Al + Fe^{3+} -> Fe + Al^{3+}}$$ happens. I guess the activation energy is very high, because you need to split the $$Fe_2O_3$$$$\ce{Fe_2O_3}$$ into $$Fe^{3+}$$$$\ce{Fe^{3+}}$$ and $$O^{2-}$$$$\ce{O^{2-}}$$. Probably you need molten aluminium too at 660°C$$\pu{660°C}$$ to ignite it.

I was wondering whether it is possible to ignite thermite in a water solution. Since $$O^{2-} + H_2O \rightarrow 2OH^-$$$$\ce{O^{2-} + H_2O -> 2OH^-}$$, I guess a very acidic solution could help to start the reaction, since $$OH^- + H^+ = H_2O$$$$\ce{OH^- + H^+ <=> H_2O}$$. On the other hand it could mean a $$2Al + 6H^{+} \rightarrow 2Al^{3+} + 3H_2\uparrow$$$$\ce{2Al + 6H^{+} \rightarrow 2Al^{3+} + 3H_2\uparrow}$$ reaction too.

Any idea whether thermite can be ignited this way, for example with a drop of concentrated acid? Or will it just result hydrogen gas, because that reaction has a lot lower activation energy?

As far as I know thermite is a typical redox reaction where $$Al + Fe^{3+} \rightarrow Fe + Al^{3+}$$ happens. I guess the activation energy is very high, because you need to split the $$Fe_2O_3$$ into $$Fe^{3+}$$ and $$O^{2-}$$. Probably you need molten aluminium too at 660°C to ignite it. I was wondering whether it is possible to ignite thermite in a water solution. Since $$O^{2-} + H_2O \rightarrow 2OH^-$$, I guess a very acidic solution could help to start the reaction, since $$OH^- + H^+ = H_2O$$. On the other hand it could mean a $$2Al + 6H^{+} \rightarrow 2Al^{3+} + 3H_2\uparrow$$ reaction too. Any idea whether thermite can be ignited this way, for example with a drop of concentrated acid? Or will it just result hydrogen gas, because that reaction has a lot lower activation energy?

As far as I know thermite is a typical redox reaction where $$\ce{Al + Fe^{3+} -> Fe + Al^{3+}}$$ happens. I guess the activation energy is very high, because you need to split the $$\ce{Fe_2O_3}$$ into $$\ce{Fe^{3+}}$$ and $$\ce{O^{2-}}$$. Probably you need molten aluminium too at $$\pu{660°C}$$ to ignite it.

I was wondering whether it is possible to ignite thermite in a water solution. Since $$\ce{O^{2-} + H_2O -> 2OH^-}$$, I guess a very acidic solution could help to start the reaction, since $$\ce{OH^- + H^+ <=> H_2O}$$. On the other hand it could mean a $$\ce{2Al + 6H^{+} \rightarrow 2Al^{3+} + 3H_2\uparrow}$$ reaction too.

Any idea whether thermite can be ignited this way, for example with a drop of concentrated acid? Or will it just result hydrogen gas, because that reaction has a lot lower activation energy?

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# Can you ignite the thermite reaction in a solution?

As far as I know thermite is a typical redox reaction where $$Al + Fe^{3+} \rightarrow Fe + Al^{3+}$$ happens. I guess the activation energy is very high, because you need to split the $$Fe_2O_3$$ into $$Fe^{3+}$$ and $$O^{2-}$$. Probably you need molten aluminium too at 660°C to ignite it. I was wondering whether it is possible to ignite thermite in a water solution. Since $$O^{2-} + H_2O \rightarrow 2OH^-$$, I guess a very acidic solution could help to start the reaction, since $$OH^- + H^+ = H_2O$$. On the other hand it could mean a $$2Al + 6H^{+} \rightarrow 2Al^{3+} + 3H_2\uparrow$$ reaction too. Any idea whether thermite can be ignited this way, for example with a drop of concentrated acid? Or will it just result hydrogen gas, because that reaction has a lot lower activation energy?