# What are the oxidation and reduction equations for when zinc is placed in HCl?

Jul 10, 2017

Zinc is oxidized to $Z {n}^{2 +}$.........

#### Explanation:

$Z n \left(s\right) \rightarrow Z {n}^{2 +} + 2 {e}^{-}$ $\left(i\right)$

And hydronium ion is REDUCED to dihydrogen gas.........

${H}_{3} {O}^{+} + {e}^{-} \rightarrow \frac{1}{2} {H}_{2} \left(g\right) + {H}_{2} O \left(l\right)$ $\left(i i\right)$

And we add the equations together to eliminate the electrons.....

$Z n \left(s\right) + 2 {H}_{3} {O}^{+} \rightarrow Z {n}^{2 +} + {H}_{2} \left(g\right) \uparrow + 2 {H}_{2} O \left(l\right)$

And since chloride anion is conceived to be a spectator in this reaction.....

$Z n \left(s\right) + 2 H C l \left(a q\right) \rightarrow Z n C {l}_{2} \left(a q\right) + {H}_{2} \left(g\right) \uparrow$

Is mass balanced? Is charge balanced? If the answer is NO, then the reaction cannot be considered to represent reality.