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------------------------------------------------ When 1.57 mol of [tex]O_2[/tex] reacts with [tex]H_2[/tex] to form [tex]H_2O[/tex], how many moles of [tex]H_2[/tex] are consumed in the process?

A. 1.57 mol
B. 0.785 mol
C. 3.14 mol
D. 2.36 mol

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.