Magnesium And Oxygen Conjoin In A Whole-Number Ratio

Weigh the large block on an electronic balance and write the mass on the data table. Record the masses of the metal blocks in grams and maintain the certainty of either the milligram or analytical balance. When you are finished recording show your data to your instructor for their initials.

Hypothesis/Prediction: The percent composition by mass of magnesium in magnesium oxide will not change significantly with each group that conducted the experiment. The composition of each substance should stay the same and any differences must be due to some error.

2. Used a test tube clamp to held the test tube and gently heated the tube in a laboratory burner flame for about 30 seconds.

red powder, heating it, weighing it, reheating it, and weighing it again until we reached a constant mass, we were able to determine the

5) Light the Bunsen Burner and set up the crucible above the burner so that the hottest portion of the flame touches the bottom of the crucible.

Based on my and other classmates' observations and results it can be proved that every time magnesium combines with oxygen to form Magnesium oxide the percent composition for magnesium will be 60.31% and for oxygen it will be 30.69 % (the results achieved by experiments are

In this lab, we will create a chemical reaction between the reactants oxygen (O2) and magnesium (Mg) using combustion. The product will be magnesium oxide (MgO). In this lab we will record the masses of reactants and products to perform stoichiometry of the chemical equation Mg + O2 -> MgO. The actual yield of product will differ from the theoretical yield based on how the experiment is performed. The independent variable is the product amounts and the dependent variable is the percent yield.

The next step was to heat the empty crucible. The purpose of firing the crucible is to remove any condensation, moisture, or contaminants that might be present in the crucible which could affect the measuremnets. All the measuremnts of the crucible, lid, and sample were performed at room temperature. This technique is necessary for gravimetric analysis because at room temperature the experiement is performed at a fixed state without heat and convention currents that would change the measuremnets.

) Suppose that some magnesium oxide smoke had escaped during the investigation, the Mg:O ratio would have increased from 58% to 72%. The final mass of MgO would have decreased because the magnesium oxide smoke is part of the product and when some of it escapes, it decreases the final mass.

Finally, turn off the burner and remove the sample using a crucible tong. Allow the

Repeat measuring the mass of the object three (3) more times; ensuring that the balance is re-zeroed after each measurement. Tabulate data gathered. Procedure 2: Find the mass of the object given, as done in procedure 1. Ensure that the object is dry when it is being placed on the balance, as this will yield an inaccurate reading. Get a clean 1000milliter beaker. Fill the beaker to approximately half its capacity. Note the exact volume of water placed into the beaker. When reading the volume of the water, ensure that this is done at eye level, and that it is read at the bottom of the meniscus. After noting the initial volume of water, place the object carefully into the water. DO NOT SPLASH. Note the final volume of water in the beaker. Tabulate data gathered.

Low temp for drying the sample , then the wall is heated up to 1400 K for short period to ash the sample, then up to 2550 K for few seconds to produce gas phase atoms.

Then, wait to see if the mg ribbon has turned to white ash. If it has turned to white ash, let the crucible cool and add 10 drops of distilled water. Then partially cover the crucible and heat for 10 min and then let it cool. Then after the crucible has cooled, weigh the mass of the crucible, lid, and mg ribbon inside. If the student had extra time he could reheat the crucible for 5-10 min and then let it cool down and weigh it

Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.

III. For observation 1 and 2, pour 1 cup of water into a pan and place on stove on high heat. For observation 2 add