Describe the process that was used in this lab to create magnesium oxide, specifically identifying the type of chemical reaction. Explain why the product had a higher mass than the reactant, and how this relates to conservation of matter.

Answer & Explanation:

1. The process that was used in the lab to create MgO:

Mg is weighed in a crucible and then heated in air that reacts strongly with O₂ to give MgO according to the equation:

Mg + 1/2O₂ → MgO

and this is confirmed by the increase in mass of Mg in the crucible.

2. The type of the chemical reaction:

It is considered as an oxidation reaction, thus the magnesium gain O and oxidized to MgO.

3. The reason that the product had a higher mass than the reactant:

Because the reactant (Mg) bonded to O and forms MgO, so the product had a higher mass due to the gain of O atom over the reactant Mg.

4. The relation to the conversation of matter:

The law of conversation of matter states that the matter goes not destroyed or created from nothing but it can converted from one form to other. Herein Mg and O₂ converted from their atom state to MgO fixing the presence of matter and also the conversation of mass. If we have 1.0 mole of Mg will react with 0.5 mole of O₂ to produce 1.0 mole of MgO.

The mass of Mg = n x molar mass of Mg = (1.0 mole) (24.30 g/mol) = 24.3 g.

The mass of O₂ = n x molar mass of O₂ = (0.5 mole) (32.00 g/mole) = 16.0 g.

The mass of MgO = n x molar mass of MgO = (1.0 mole) (40.30 g/mol) = 40.3 g/mol.

The mass of the reactants = The mass of Mg + The mass of O₂ = 24.3 g + 16.0 g = 40.3 g. The mass of the products = The mass of MgO = 40.3 g.

∴ The mass of the reactants = The mass of the products.

So, there is a conversation of matter and mass.