Experiment #1:%0D%0A%0D%0A%0D%0A%0D%0A %0D%0A%0D%0A(4 points)%0D%0A1. What is the mass of each reactant?%0D%0A%0D%0AMagnesium: %0D%0A44.5 g%0D%0AOxygen%0D%0A28.9 g%0D%0A2. The total mass of all the reactants is:%0D%0A73.4 g%0D%0A%0D%0A3. The total mass of the products is %0D%0A117.9 g%0D%0A%0D%0AQuestion 2%0D%0A4. Does this experimental data support the Law of Conservation of Mass? Explain in full sentences.(2 points)

Answer 1

The Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction; it means that the total mass of the reactants must equal the total mass of the products.

In your experiment, the total mass of the reactants is calculated as follows:

• Mass of Magnesium: 44.5 g
• Mass of Oxygen: 28.9 g
• Total mass of reactants = 44.5 g + 28.9 g = 73.4 g

However, you report the total mass of the products as 117.9 g. This indicates a discrepancy, since the total mass of the products should also equal 73.4 g if the Law of Conservation of Mass is upheld.

Since the mass of the products (117.9 g) does not equal the mass of the reactants (73.4 g), this experimental data does not support the Law of Conservation of Mass. There could be several reasons for this discrepancy, such as measurement errors, loss of reactants during the experiment, or gaining mass from the environment (e.g., absorptions of gases or impurities). Therefore, the results suggest that not all mass was accounted for in the reaction, conflicting with the principle that mass is conserved.