Final answer:
For the given reaction, 4.00 moles of MnO₂ and 2.00 moles of H₂O are required to react completely with 2.00 mol Zn.
Step-by-step explanation:
In the given reaction:
Zn(s) + 2 MnO₂(s) + H₂O(l) → Zn(OH)₂(aq) + Mn₂O₃(s)
The stoichiometry of the balanced equation shows that for every 1 mole of Zn, 2 moles of MnO₂ and 1 mole of H₂O are required for complete reaction.
Since there are 2.00 moles of Zn given, we can conclude that 4.00 moles of MnO₂ and 2.00 moles of H₂O are required for complete reaction.
To calculate the number of moles of MnO₂ and H₂O needed to react with 2.00 mol of Zn according to the balanced chemical equation Zn(s) + 2 MnO₂(s) + H₂O(l) → Zn(OH)₂ (aq) + Mn₂O₃(s), we use the stoichiometry of the reaction. The equation indicates that each mole of Zn reacts with 2 moles of MnO₂ and 1 mole of H₂O. Therefore, for 2.00 moles of Zn, you will need 4.00 moles of MnO₂ and 2.00 moles of H₂O to react completely.