Answer :
Final answer:
To find the moles of H₂ consumed when reacting with O₂, apply the stoichiometric ratio from the balanced equation. For 1.57 mol O₂, double the amount, 3.14 mol H₂, is needed due to a 2:1 ratio in the reaction to form H₂O (option a).
Explanation:
To determine how many moles of H₂ are consumed when 1.57 mol of O₂ reacts to form H₂O, we must look at the balanced chemical equation for the reaction:
2 H₂(g) + O₂(g) → 2 H₂O(l)
According to the stoichiometry of the reaction, it takes 2 moles of hydrogen gas (H₂) to react with 1 mole of oxygen gas (O₂) to produce 2 moles of water (H₂O). Therefore, if we have 1.57 mol of O₂, the stoichiometry tells us that twice that amount of H₂ will be needed, since the mole ratio of H₂ to O₂ is 2:1.
So, the calculation is:
- 1.57 mol O₂ × (2 mol H₂ / 1 mol O₂) = 3.14 mol H₂
The answer is 3.14 moles of H₂ are needed to react with 1.57 moles of O₂.
