The mole can be also defined as the number of atoms in exactly 12g of Carbon. In this experiment, the magnesium will be heated and this magnesium will react with the oxygen in the air to form magnesium Oxide. DIAGRAM: METHOD: 1. An empty crucible and its lid were weighed on an electrical balance. The mass of the crucible and its lid were recorded.
2. Clean the magnesium ribbon with sandpaper. 3. Coil the ribbon and place it in the crucible. Weigh the crucible with its lid and the content in it.
To work out the formula of the magnesium oxide, we need relative atomic masses and number of moles of magnesium and oxygen. By finding the moles involved in the reaction, we can work out the ratio of the magnesium to oxygen in the compound (magnesium oxide) should be 1:1. A balance formula of the experiment: 2Mg(s) + O2(g) → 2MgO(s) Method The same balance was used for the weighing in the experiment 1. All apparatus were set up. 2.
Determine the mass of a Florence flask. 2. Obtain a small piece of magnesium from the instructor and place it in the flask. Determine the mass of this entire assembly. 3.
3. Place the “R” tube in a beaker and get a large test tube, another boiling tube and a pipet. Label the large test tube “C” and the boiling tube “P”. Place one boiling chip into the “P” tube. 4.
Gravimetric Determination of Sulfate Purpose The purpose of this lab is to determine the percentage of sulfate in the hydrate by precipitating the sulfate as barium sulfate. Materials Filler paper Sodium sulfate Graduated cylinder Bunsen burner Watch glass Beakers (250 mL, 400 mL) Rubber bulb Graduated pipette Beaker tongs Funnel Filter Paper Sodium Sulfate Drying oven Wash bottle Stirring rod Silver nitrate Hydrochloric acid Distilled water Small test tube Procedures First, .4861 grams of sodium sulfate was placed into a clean 400mL beaker. Exactly 200mL of water and 1mL of HCl was added to the same beaker. A watch glass was placed on the beaker and the solution was heated using the Bunsen burner to a gentle boil. The watch glass was removed with the beaker tongs.
* Dispose of any solid residue as directed by your instructor. Procedure Measure the mass of the crucible with its lid on the electric balance. Record your data. Loosely fold the Magnesium ribbon and put in the crucible. Measure their mass on the electric balance.
Thermodynamics and Kinetics of Carbonates 3/31/2014 Experimentally it was determined that with the presence of magnesium in solution, aragonite readily transforms to calcite. By analyzing the data collected by Group 7 (Friday Lab 2) it can be concluded that the presence of magnesium acts as an inhibitor for the aragonite – magnesium transformation. 1.0 Introduction The objective of this lab is to practically apply knowledge of thermodynamics and kinetics. A stronger understand of X-Ray Diffraction (XRD) measurements will also be gained. Laboratory 2/3 will follow the rate at which aragonite transforms to calcite.
A magnesium piece of metal was obtained and cut in to five pieces. It was then weighed and recorded with the crucible and lid on it. Tongs were used to carefully place the crucible on the wire gauze and the lid was placed three fourths of the way on it. The crucible was heated for twelve minutes on high heat. DO NOT LOOK DIRECTLY AT THE BURNING MAGNESIUM; THE INTENSE LIGHT CAN HURT YOUR EYES.
Note: The experiment was done at room temperature and not 0 degrees so of course , the result will be different than the one known, which is 300000 j/kg , but as the main point of this experiment is to see if latent heat changes with the change of time , so it won’t affect the experiment . Results : Set A: Time = 3 minutes = 180 seconds Voltage(v) | Current(A) | Weight of empty beaker (kg) | Weight of beaker after melting of ice (kg) | Weight difference | Heat Energy (J) | Latent Heat (J/kg) | 12V | 2.17A | 0.398 kg | 0.404 kg | 0.006 kg | 4687.2 J | 781200 j/kg | Set B: Time = 2minutes = 120 seconds Voltage(v) | Current(A) |