Dear beloved readers, welcome to our website! We hope your visit here brings you valuable insights and meaningful inspiration. Thank you for taking the time to stop by and explore the content we've prepared for you.
------------------------------------------------ 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

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.