Show your calculations for each of the following. Remember, calculations should follow rules for significant figures.

1. Write the balanced chemical equation for the reaction you are performing.
2. Calculate the mass of magnesium metal used in each trial.
Trial 1:
Trial 2:

3. Calculate the actual yield of magnesium oxide for each trial.
Trial 1:
Trial 2:

4. Magnesium is the limiting reactant in this experiment. Calculate the theoretical yield of MgO for each trial.
Trial 1:
Trial 2:

5. Determine the percent yield of MgO for your experiment for each trial.
Trial 1:
Trial 2:
6. Determine the average percent yield of MgO for the two trials.

Questions and Conclusions:
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.

What sources of error may have contributed to the percent yield not being 100 percent? Think about things that may have led to inaccurate measurements or where mass of the product could have been lost if this experiment was conducted in a physical laboratory.

When conducting this experiment, some procedures call for heating the substance several times and recording the mass after each heating, continuing until the mass values are constant. Explain the purpose of this process and how it might reduce errors.

Your company currently uses a process with a similar cost of materials that has an average percent yield of 91 percent. If the average percent yield of this process is higher than that, this could save the company money. What is your recommendation to the company? Please support your recommendation using your data, calculations, and understanding of stoichiometry gathered from this lab.

Data
Mass of empty crucible with lid
Trial 1 26.682g
Trial 2 26.683g
Mass of Mg metal, crucible, and lid
Trial 1 27.176g
Trial 2 27.105g
Mass of MgO, crucible, and lid
Trial 1 26.984g
Trial 2 26.940g