Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s}) \rightarrow \mathrm{Fe}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) $$

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To balance the chemical equation $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s}) \rightarrow \mathrm{Fe}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) $$, we will follow these steps:

1. **Identify the number of atoms of each element on both sides of the equation.**
   - On the left side (reactants), we have:
     - Iron (Fe): 2 (from $$ \mathrm{Fe}_{2} \mathrm{O}_{3} $$)
     - Oxygen (O): 3 (from $$ \mathrm{Fe}_{2} \mathrm{O}_{3} $$)
   - On the right side (products), we have:
     - Iron (Fe): 1 (from $$ \mathrm{Fe} $$)
     - Oxygen (O): 2 (from $$ \mathrm{O}_{2} $$)

2. **Balance the iron (Fe) atoms first.**
   - Since there are 2 Fe atoms on the left, we need 2 Fe atoms on the right. We can do this by placing a coefficient of 2 in front of $$ \mathrm{Fe} $$:
   $$
   \mathrm{Fe}_{2} \mathrm{O}_{3} \rightarrow 2 \mathrm{Fe} + \mathrm{O}_{2}
   $$

3. **Now, balance the oxygen (O) atoms.**
   - On the left, we have 3 O atoms, and on the right, we have 2 O atoms from $$ \mathrm{O}_{2} $$. To balance the oxygen, we can place a coefficient of $$ \frac{3}{2} $$ in front of $$ \mathrm{O}_{2} $$:
   $$
   \mathrm{Fe}_{2} \mathrm{O}_{3} \rightarrow 2 \mathrm{Fe} + \frac{3}{2} \mathrm{O}_{2}
   $$

4. **Convert to whole number coefficients.**
   - To eliminate the fraction, we can multiply the entire equation by 2:
   $$
   2 \mathrm{Fe}_{2} \mathrm{O}_{3} \rightarrow 4 \mathrm{Fe} + 3 \mathrm{O}_{2}
   $$

Now, the balanced equation with the smallest possible whole number stoichiometric coefficients is:
$$
\boxed{2 \mathrm{Fe}_{2} \mathrm{O}_{3} \rightarrow 4 \mathrm{Fe} + 3 \mathrm{O}_{2}}
$$
The balanced chemical equation is: $$ 2 \mathrm{Fe}_{2} \mathrm{O}_{3} \rightarrow 4 \mathrm{Fe} + 3 \mathrm{O}_{2} $$

Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s}) \rightarrow \mathrm{Fe}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \)

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