Balance the oxidation reaction of iron rusting: 4Fe + 3O2 -> 2Fe2O3 with oxidation states and atom conservation.
Use uppercase and lowercase symbols properly (e.g. Fe for iron, not FE). Separate with + and -> or =.
| Element | Reactant Atoms (Left) | Product Atoms (Right) | Status |
|---|
Formulated by Antoine Lavoisier in 1789, the Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction. The atoms present in the reactants are simply rearranged to form new products. Consequently, the mass of the reactants must exactly equal the mass of the products.
4Fe + 3O₂ → 2Fe₂O₃ (Iron(III) Oxide)
| Reaction Name | Unbalanced Formula | Balanced Equation | Reaction Type |
|---|---|---|---|
| Photosynthesis | CO2 + H2O -> C6H12O6 + O2 | 6CO2 + 6H2O -> C6H12O6 + 6O2 | Synthesis / Endothermic |
| Cellular Respiration | C6H12O6 + O2 -> CO2 + H2O | C6H12O6 + 6O2 -> 6CO2 + 6H2O | Combustion / Exothermic |
| Methane Combustion | CH4 + O2 -> CO2 + H2O | CH4 + 2O2 -> CO2 + 2H2O | Complete Combustion |
| Rusting of Iron | Fe + O2 -> Fe2O3 | 4Fe + 3O2 -> 2Fe2O3 | Oxidation / Synthesis |
| Water Synthesis | H2 + O2 -> H2O | 2H2 + O2 -> 2H2O | Combination Reaction |
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