How many grams of water can be produced from 4.6 grams of Hydrogen and 7.3 grams of Oxygen?

H2 + O2 —> H2O

The answer to your question is 8.21 g of H₂O

Explanation:

Data

mas of water = ?

mass of hydrogen = 4.6 g

mass of oxygen = 7.3 g

Balanced chemical reaction

                   2H₂  +  O₂  ⇒   2H₂O

Process

1.- Calculate the atomic mass of the reactants

Hydrogen = 4 x 1 = 4 g

Oxygen = 16 x 2 = 32 g

2.- Calculate the limiting reactant

Theoretical yield = H₂/O₂ = 4 / 32 = 0.125

Experimental yield = H₂/ O₂ = 4.6/7.3 = 0.630

From the results, we conclude that the limiting reactant is Oxygen because the experimental yield was higher than the theoretical yield.

3.- Calculate the mass of water

                   32 g of O₂ 36 g of water

                   7.3 g of O₂   x

                          x = (7.3 x 36) / 32

                          x = 262.8 / 32

                          x = 8.21 g of H₂O

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

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