If 50.0 g of h2 and 100.0 g of o2 react, how
many moles of h2o can be produced in the
reaction below?
2 h2(g) + o2(g) → 2 h2o(g)

The number of mole of H₂O produced from the reaction between 50 g of H₂ and 100 g of O₂ is 6.25 moles.

We'll begin by calculating the number of mole in 50 g of H₂ and 100 g of O₂. This can be obtained as follow:

Mass of H₂ = 50

Molar mass of H₂ = 1 × 2 = 2 g/

Mole = mass / molar mass

Mole of H₂ = 50 / 2

Mass of O₂ = 100

Molar mass of O₂ = 16 × 2 = 32 g/

Mole = mass / molar mass

Mole of O₂ = 100 / 32

         2H₂  +  O₂  —>  2H₂O

        2     :     1

       25    :     3.125

From the above, we can see that O₂ is the limiting reactant and H₂ is the excess reactant since a lesser amount of O₂ is present.

From the balanced equation above,

1 mole of O₂ reacted to produce 2 moles of H₂O.

Therefore,

3.125 moles of O₂ will react to produce = 3.125 × 2 = 6.25 moles of H₂O.

Thus, the number of mole of H₂O produced from the reaction is 6.25 moles.

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6.25 moles

Explanation:

Given data:

Mass of H₂ = 50 g

Mass of O₂ = 100 g

Moles of H₂O = ?

Chemical equation:

O₂  + 2H₂  → 2 H₂O

Number of moles of H₂:

Number of moles of  H₂= Mass /molar mass

Number of moles of H₂= 50 g / 2/mol

Number of moles of  H₂= 25 mol

Number of moles of O₂  :

Number of moles of O₂  = Mass /molar mass

Number of moles of O₂  = 100g / 32 g/mol

Number of moles of O₂  = 3.125 mol

Now we will compare the moles of water with hydrogen and oxygen .

                  O₂             :            H₂ O

                   1               :               2

                 3.125         :            2 × 3.125 =6.25

                  H₂             :                H₂O

                   2              :                 2

                 25             :                  25

The number of moles of H₂O produced by oxygen are less it will be limiting reactant.

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