# Question #df03f

Jul 19, 2017

${\text{Si"_ ((s)) + 2"H"_ 2"O"_ ((g)) -> "SiO"_ (2(s)) + 2"H}}_{2 \left(g\right)} \uparrow$

#### Explanation:

Red hot silicon will react with steam to produce silicon oxide and hydrogen gas.

The balanced chemical equation that describes this reaction looks like this

${\text{Si"_ ((s)) + 2"H"_ 2"O"_ ((g)) -> "SiO"_ (2(s)) + 2"H}}_{2 \left(g\right)} \uparrow$

Notice that this is actually a redox reaction in which silicon is being oxidized to silicon oxide and water is being reduced to hydrogen gas.

${\stackrel{\textcolor{b l u e}{0}}{\text{Si") _ ((s)) + 2 stackrel(color(blue)(+1))("H") _ 2"O"_ ((g)) -> stackrel(color(blue)(-2))("Si") "O"_ (2(s)) + stackrel(color(blue)(0))("H}}}_{2 \left(g\right)}$

As it turns out, it would be possible to have a reaction between silicon and water at temperatures as low as room temperature $\to$ see this reference for more info on that.