Question

In the reaction represented by the equation 2Na + 2H2O -------> 2NaOH + H2, how many grams of hydrogen are produced if 120. g of Na and 80.0 g of H2O are available?

Answer 1

The answer to your question is 177.8 g of NaOH

Step-by-step explanation:

Balanced chemical reaction

2 Na + 2 H₂O ⇒ 2 NaOH + H₂

Data

Grams of H₂ = ?

Mass of Na = 120 g

Mass of H₂O = 80

Process

1.- Calculate the limiting reactant

Molar mass of Na = 2 x 23 = 46 g

Molar mass of H₂O = 2 x 18 = 36 g

Theoretical proportion Na/H₂O = 46/36 = 1.28

Experimental proportion Na/H₂O = 120/80 = 1.5

As the experimental proportion increases, we conclude that the limiting reactant is the water.

2.- Calculate the mass of hydrogen

Molar mass of NaOH = 2[23 + 16 + 1] = 80 g

36 g of H₂O ------------------ 80 g of NaOH

80 g of H₂O ----------------- x

x = (80 x 80) / 36

x = 6400 / 36

x = 177.8 g of NaOH