Ask Question
10 February, 20:22

When 1.57 mol o2 reacts with h2 to form h2o, how many moles of h2 are consumed in the process?

+5
Answers (2)
  1. 10 February, 21:22
    0
    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.
  2. 11 February, 00:06
    0
    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.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “When 1.57 mol o2 reacts with h2 to form h2o, how many moles of h2 are consumed in the process? ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers