# What are the reducing and oxidizing agents in the equation? If there are none, write “no redox reaction" (include oxidation states for each element in the equation)

Apr 29, 2017

$\text{Ferric ion}$ is reduced..........

#### Explanation:

And $\text{oxalate ion}$ is oxidized to carbon dioxide.

$\text{Reduction half equation:}$

$F {e}^{3 +} + {e}^{-} \rightarrow F {e}^{2 +}$ $\left(i\right)$

$\text{Oxidation half equation:}$

""^(+III)C_2O_4^(2-) rarr 2CO_2 +2e^(-) $\left(i i\right)$

For each equation, MANIFESTLY, both charge and mass are balanced, as they must be if they reflect chemical reality, and the final redox equation takes $2 \times \left(i\right) + \left(i i\right) :$

$2 F {e}^{3 +} + {C}_{2} {O}_{4}^{2 -} \rightarrow 2 F {e}^{2 +} + 2 C {O}_{2} \left(g\right) \uparrow$

Are charge and mass balanced here? Don't trust my arithmetic!