The powder that remains will have lost some mass as smoke, but this resultant mass is still more than the mass of the metal that was burnt. Burning magnesium in air is a chemical reaction called oxidation and the compound produced is totally different from the two elements that have been combined. Each element is made up of atoms and the compound is made up of two elements joined together. The chemical formula for the reaction is below; 2Mg + O2 --> 2MgO Magnesium + Oxygen -> Magnesium Oxide The equation above shows that magnesium and oxygen have combined as the product of the reaction, their mass of each element has also combined in the reaction. Magnesium is a very reactive metal which when heated burns with a white flame.
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.
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.
Determining the Empirical Formula of Magnesium Oxide Lab Purpose The purpose of this lab was to determine the percent composition and empirical formula of magnesium oxide. Hypothesis If a strip of pure magnesium metal reacts with oxygen in the air to create magnesium oxide, then the molecular formula will be MgO. The percent composition for magnesium oxide would be 60.31% magnesium and 39.69% oxygen. Apparatus Refer to attached sheet Procedure Refer to McGraw-Hill Ryerson Chemistry 11, page 212-213. 4.
The reactions are different because ethanoic acid has weaker attractions and gives away the electron in its outer shell easier. We didn't have time to see the volume of hydrogen being the same. Evaluation I believe that the precision of our measurements of acid could've been better. Using glass beakers with a higher resolution would allow us to correctly measure the amount of acid we would be reacting. Also, we lacked precision in timing, and should've used a more precise stopwatch to make sure it was a fair test.
Prepare the apparatus according to diagram A. 2. Prepare 100 cm3 of 0.2 M hydrochloric acid by mixing 10 cm3 of 2 M hydrochloric acid with 90 cm3 of distilled water. 3. Fill the conical flask with 50 cm3 of 0.2 M hydrochloric acid.
The Empirical Formula of an Oxide, Purpose: The purpose of this lab was to determine the empirical formula of magnesium oxide. To do this, we measured the weight of the magnesium before the reaction with oxygen, and then measure it after it had bonded with the oxygen. After the mass of the items were collected, the data was calculated in empirical formula. Background: The empirical formula of a compound is the whole number ratio of the elements in a compound. For example, the empirical formula of water is H2O meaning for every 1 O atom there are 2 H atoms.
Purpose What happens to the speed of a reaction between Calcium Carbonate (CaCO3 1M & 3M) and Hydrochloric acid (HCl) as the temperature is changed and the surface area of the reactant. HCl(aq) + CaCO3(s) → CaCl2(aq) + CO2(g) + H2O(l) is the reaction. Hypothesis Factors affecting the rate of Chemical reactions are varied. The “Rate of Reaction” means how fast is the reaction. In the collision theory reactions can happen when the reactant particles collide successfully but most collisions are not successful.
Heat is needed to start and continue a fire. The heat causes the fuel to break down in a process called pyrolysis, in which the fuel is taken from a solid state of matter to a gaseous state. It is the gasses that burn, not the solid or liquid matter. The next part of the fire triangle is oxygen. Oxygen is not actually pure oxygen; it’s the ambient air which is roughly 15-21% oxygen, depending on altitude and pollution.
Si, P, S and Cl are increasingly electronegative. They cannot form oxide ions from oxygen at all, so they behave as acids. The trend is from strongly basic oxides on the left-hand side to strongly acidic ones on the right, via an amphoteric oxide (aluminium oxide) in the middle. In addition, when going across the period 3 the acid-base nature of the oxides change from base to amphoteric and finally to become acid. This is because the less electronegative sodium has a weak Na-O bond and the oxygen is more easily given up to reacts with H+.