Final answer:
The balanced chemical equation for the reaction of manganese (Mn) with oxygen (O₂) to form manganese(IV) oxide is typically 3 Mn (s) + 2 O₂ (g) → Mn₃O₄ (s). However, for exactly 5 moles of Mn and 5 moles of O₂.
Step-by-step explanation:
The reaction between manganese (Mn) and oxygen (O₂) to form manganese(IV) oxide can be represented by the balanced chemical equation Mn + O₂ → MnO₂. To determine the balanced equation from 5 mol of Mn and 5 mol of O₂, we need to account for the stoichiometry of the reaction. However, the question appears to have a mistake, as the given chemicals and equations in the references talk about manganese in different oxidation states reacting in solution, not solid manganese reacting with oxygen gas, which would be a synthesis reaction to form an oxide.
Assuming instead that we are looking for the reaction of solid manganese with oxygen gas, typically, Mn reacts with O₂ in a ratio where 3 moles of Mn reacts with 2 moles of O₂ to form Mn₃O₄. The balanced equation for the reaction of Mn with O₂ would then be:
- 3 Mn (s) + 2 O₂ (g) → Mn₃O₄ (s)
This indicates that with 5 moles of Mn and 5 moles of O₂, there would be an excess of O₂ since the stoichiometric ratio is not 1:1. To fully react 5 moles of Mn, 3.33 moles of O₂ would be required, and the remaining O₂ would be in excess. The balanced equation above is not applicable for precisely 5 moles of each reactant.