10. A 3.192 gram sample of magnesium sulfate was heated in a beaker. 10 minutes after heating was completed, the mass of the sample was 1.559g. No chemical reaction occurred. What is the molecular formula for the sample of magnesium sulfate that was heated? Show all work. (5 pts)
11. The empirical formula of a compound is C3H2O. If the molar mass of the compound is found to be 216 g/mol, find the molecular formula (true formula). You must show all work with the units.
(3 pts)
12. Determine the empirical formula of the following compound if a sample contains 55.80 % carbon, 7.038 % hydrogen, and 37.17 % oxygen by mass. You must show all work with the units.

Which statement describes both homogeneous mixtures and heterogeneous mixtures?

These questions are based on the attached photo. the experiment is about burning magnesium metal with oxygen. 1. write the balanced chemical equation for the reaction you are performing. 2. calculate the mass of magnesium metal used in each trial. o trial 1: o trial 2: 3. calculate the actual yield of magnesium oxide for each trial. o trial 1: o trial 2: 4. magnesium is the limiting reactant in this experiment. calculate the theoretical yield of mgo for each trial. o trial 1: o trial 2: 5. determine the percent yield of mgo for your experiment for each trial. o trial 1: o trial 2: 6. determine the average percent yield of mgo for the two trials. 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? support your recommendation using your data, calculations, and understanding of stoichiometry gathered from this lab.

What was bohr’s contribution to the planetary model