# How hydrochloric acid reduce PbCl_4 to lead metal, and oxidize chloride to chlorine gas?

Apr 10, 2017

$P b {O}_{2} \left(s\right) + 4 H C l \left(a q\right) \rightarrow P b C {l}_{2} \left(s\right) + 2 {H}_{2} O \left(l\right) + C {l}_{2} \left(g\right)$

#### Explanation:

$P \left(+ I V\right)$ is reduced to $P b \left(+ I I\right)$:

$P {b}^{4 +} + 2 {e}^{-} \rightarrow P {b}^{2 +}$ $\left(i\right)$

Chloride ion is oxidized to chlorine gas:

$C {l}^{-} \rightarrow \frac{1}{2} C {l}_{2} \left(g\right) + {e}^{-}$ $\left(i i\right)$

And thus $\left(i\right) + 2 \times \left(i i\right) :$

$P {b}^{4 +} + 2 C {l}^{-} + 2 {e}^{-} \rightarrow P {b}^{2 +} + C {l}_{2} \left(g\right) + 2 {e}^{-}$

Which is balanced with respect to mass and charge.

We can write a more conventional stoichiometric equation, by substituting the ions for the parent compounds.......

$P b {O}_{2} + 4 H C l \rightarrow P b C {l}_{2} \left(s\right) \downarrow + C {l}_{2} \left(g\right) \uparrow + 2 {H}_{2} O$

Is this balanced with respect to mass and charge?