Problem Statement: Through this experiment mass relationships between reactants and products will be formulated by heating the reactant and observing the reaction taking place. This investigation involves finding the mass relationships of the initial and final mass by burning magnesium. Materials: Bunsen burner Striker Crucible Tongs / tweezers Analytical Balance Goggles Safety- Wear goggles at all time. Keep burning reaction pointing away from face In this investigation, data will be collected from the observations of the mass relationship when magnesium is burned. An initial and final mass will be taken using an analytical balance. Using this date, a % yield will be determined to show the mass relationships when magnesium is burned.
Procedure: 1. Obtain a piece of magnesium from the instructor and record the mass by using the Analytical balance. 2. Next weight the crucible and record its mass, if desired the magnesium can be weighed with the crucible and at the end subtract the mass of the crucible itself giving the mass of the magnesium itself.
3. Observe the composition of the magnesium as well has its physical properties then record. 4. Place the crucible with the piece of magnesium in it on the ring stand. 5.
Next light the Bunsen burner using the striker making sure the gas does not leak to long while trying to ignite. 6. Adjust the flame using the air valve to get a pure blue flame with a medium height 7. Observe the reaction of the magnesium under the flame and record details. 8.
'Aim. To find out the empirical formulae for magnesium-oxide Introduction. The empirical formula of a compound tells us the types of atoms present in a compound as well as the simplest whole-number ratio of the different types of atoms. The empirical formula does not tell us the actual number of atoms in the molecule. The mass of Mg + the mass of O 2 = mass of Mg xOx. Knowing the mass of magnesium ...
After observing the reaction taken place and everything is cool in temperature, take the crucible with the magnesium and check the mass. 9. Record the final mass and check the difference 10. Determine the % yield by using the formula actual / theoretical after calculating the theoretical mass.
11. Repeat these same steps creating 2 other trials and record data. 12. Write a formula which you think occurred during the process of this reaction.