This is a stoichiometry lab Data Observations
Create an organized data table for each part of the lab. A graph is not required for this lab report.
Mass of Magnesium
0.2443
Mass of Magnesium Oxide
0.2442

Results
Show all calculations performed as you answer the following:
A. Write the balanced equation for the reaction conducted in this lab.
B. Determine the Percent Yield:
Calculate Theoretical Yield: Use stoichiometry to calculate the expected mass of product (theoretical yield) that could be produced from the given amount of magnesium reacting with excess oxygen gas.
Calculate Percent Yield: Determine the percent yield of the reaction using the following equation:
Percent yield = Actual mass of product produced/ Theoretical yield of product × 100
C. Verify the Empirical Formula of the Product:
We are assuming that we know the formula of magnesium oxide formed. Help verify that by determining the empirical formula of the product.
Identify the mass of product formed in your experiment, MgxOy.
Identify the mass of Mg that is in the product formed.
Calculate the mass of O that is in the product.
Use the mass values to determine the mole ratio and empirical formula of the product.
Conclusion Questions
Be sure to address the following questions in the conclusion section of your report:
What was the percent yield of your reaction?
What was the limiting reactant in this experiment? How can you tell?
Why is the balanced chemical equation important in your calculation to determine the experimental yield (the actual amount of product produced in your experiment)
Is it possible to determine the percent yield of a reaction without a balanced equation, and only using mass values of the reactant and product? Explain your answer.
How were you able to determine the amount of oxygen that ended up in the product?
Did the empirical formula you calculated match with the product you predicted?