how many moles of oxygen (molecule) are required for complete reaction with 2.1080 moles of iron?
It depends upon the equation. If you form FeO, then
2Fe + O2 -->2FeO
2.1080 moles Fe x (1 mole O2/2 mols Fe) = 2.1080 x (2/1) = ??
To determine the number of moles of oxygen molecules required for a reaction with a given amount of iron, we need to first identify the balanced chemical equation for the reaction between iron and oxygen. Let's assume it is the following equation:
4Fe + 3O₂ → 2Fe₂O₃
From the balanced equation, we can see that it takes 3 moles of oxygen (O₂) to react with 4 moles of iron (Fe). This indicates a mole ratio of 3:4 between oxygen and iron.
Given that we have 2.1080 moles of iron, we can use this ratio to find the number of moles of oxygen required:
Moles of Oxygen = (2.1080 moles of Fe) × (3 moles of O₂ / 4 moles of Fe)
Performing the calculation:
Moles of Oxygen = (2.1080) × (3 / 4) ≈ 1.5810 moles of O₂
Therefore, approximately 1.5810 moles of oxygen molecules are required for the complete reaction with 2.1080 moles of iron.