Here we have to get the moles of hydrogen (H₂) consumed to form water (H₂O) from 1.57 moles of oxygen (O₂)
In this process 3.14 moles of H₂ will be consumed.
The balanced reaction between oxygen (O₂) and hydrogen (H₂); both of which are in gaseous state to form water, which is liquid in nature can be written as-
2H₂ (g) + O₂ (g) = 2H₂O (l).
Thus form the equation we can see that 1 mole of oxygen reacts with 2 moles of hydrogen to form 2 moles of water.
So, 1.57 moles of oxygen will consume (1.57×2) = 3.14 moles of hydrogen to form water.
The reaction showing the synthesis of water from its elements:
2H₂ + O₂ --> 2H₂O
One mole of oxygen combines with 2 moles of hydrogen to form 1 mole of H₂O
If 1 mole O₂ consumes 2 moles H₂
then 1.57 moles of O₂ consumes = 1.57 x 2 moles of H₂
= 3.14 moles of H₂
Therefore, 3.14 moles of H₂ are consumed in the process.
