Magnesium gives up two electrons to oxygen atoms to form this powdery product which is a form of synthesis reaction. Balanced chemical equation ---- 2 Mg (s) + O2 (g) → 2 MgO (s) Couple of changes should occur after the magnesium is burned and magnesium oxide is formed. The mass of the magnesium should increase after the process of burning and becoming magnesium oxide. The increase in mass is due to the fact that oxygen from the air has combined with the magnesium to make magnesium oxide and that will cause a combination between the mass of the oxygen and the mass of the magnesium that is used in the experiment.
The Formula of Magnesium Oxide Aim:- To find the empirical formula of magnesium oxide by burning a weighted amount of magnesium ribbon in air. Data collection, processing and presentation:- Qualitative Data: Before the magnesium strip was put in the crucible to react with oxygen it was a silverly shiny solid. when the magnesium started reacting with oxygen it changed color, but all that was seen was a white flash. As the reaction continued a white solid powder started forming around the magnesium and was soon starting to spread out all over the crucible. The ending result was some left over magnesium, that at this point was white, and the white solid powder that covered the crucible on all sides.
Experimental First, we weighed 2 samples, each has 1 gram of NaHCO3-KCl mixture Second, we put the samples in 2 crucibles (A and B) and weighed them. (crucible + sample; WA1 and WB1) Third, we heated both samples on a hot plate for 30 minutes. Fourth, we weighed the samples again (crucible + sample; WA2 and WB2) Lastly, we determined NaHCU3 percentage in the mixture using the following method: WA1 – WA2 x 100% 0.309 WA1 – WA2 x 100% 0.309 * * Results * Theorectically: * Discussion When sodium hydrogen carbonate is heated, new products are formed; sodium carbonate, water vapor, and carbon dioxide gas. This reaction may be presented in a different form with a measure of molecules: @Na2CO3 + H2O + CO2 (solid) (solid) (gas) (gas). Once the reaction of sodium hydrogen carbonate takes place, carbon dioxide gas is released, as well as water vapor.
Contents Abstract – Page 2 Summary of Results – Page 3 Focus Question – Page 5,6 What if… - Page 6 Confidence Report – Page 7,8 Abstract Summary of Results Observations of Reactions – Trials 1 , 2 & 3 | Dissolving Barium Iodide and Zinc Sulfate in deionized water | As the substances dissolve the water becomes cloudy and acquired a white tint. | Centrifuging up the solution obtained in previous reaction | The precipitate and the liquid seperated, and there was more precipitate in one of the test tubes. The precipitate was a thick white color, not transparent. | Heating the Precipitate in a boiling tube containing 2 boiling chips | The mixture began producing a large amount of bubbles, as we continued heating it only white powder remained. | Observations of Chemicals | Zinc Sulfate | Powder of a white solid | Barium Iodide | Powder of a white solid.
Observations: * Solution turns green and bubbles * Warm to the touch * Brown gas produced * Copper Dissolves Reaction 2: Copper (II) Nitrate with Sodium Hydroxide Cu(NO3)2(aq) + 2NaOH(aq) Cu(OH)2(s) + 2NaNO3(aq) Net ionic: Cu2+(aq) + 2OH-(aq) Cu(OH)2(s) Type of Reaction: Precipitate Reaction Observations: * With addition of water, the solution becomes blue, thick, and slime-like * When added to litmus paper, paper turns dark blue * Dark blue shows that the solution is basic Reaction 3: Heating Copper Cu(OH)2(s) CuO(s) + H2O(l) Net ionic: Cu(OH)2(s) CuO(s) + H2O(g) Type of Reaction: Redox Reaction: Cu is oxidized from 2- to 2+. The reducing agent is Cu(OH)3 Observations: * While heating and stirring, solution turns greyish blue, then becomes black * Cool water mixes, solution settles to the bottom * *NOT ALL WATER WAS POURED OFF Reaction 4: Copper (II) Oxide with Sulfuric Acid CuO(s) + H2SO4(aq) CuSO4(aq) +
Is There a Change in Temperature when an Alkali Neutralizes an Acid? Aim The aim of the experiment was to find out if there was a change in temperature when we added an alkali (Sodium Hydroxide) to an acid (Hydrochloric Acid) to neutralize it. Hypothesis We hypothesized that there was going be a raise in temperature as we add 1ml of Sodium Hydroxide at a time to the Hydrochloric Acid due to the neutralization of the acid. The neutralization is chemical reaction that causes an exothermic reaction. Sodium Hydroxide + Hydrochloric Acid Sodium Chloride + Water NaOH(aq) + HClaq → NaCl(aq) + H2O(l) Variables Independent The independent variable of the experiment was the amount of sodium hydroxide that we added to the acid.
a. dissolution of a penny in nitric acid b. the condensation of water vapor c. a burning candle d. the formation of polyethylene from ethylene e. the explosive reaction of hydrogen with oxygen, which produces water, | | Save Answer | | 3. (Points: 5.4) | | Which one of the following is a pure substance? a. concrete b. wood c. salt water d. elemental copper e. milk | | Save Answer | | 4. (Points: 5.4) | | Of the following, only __________ is a chemical reaction. a. melting of lead b. dissolving sugar in water c. tarnishing of silver d. crushing of stone e. dropping a penny into a glass of water | | Save Answer | | 5.
Determining the Chemical Formula of a Hydrate Purpose: Find the molecular formula of the hydrate of Copper (II) Sulfate. Materials: * 400 mL beaker * Tongs * Scoopula * Electronic Balance * Glass Rod * Hot Pad * 3 g hydrated copper(II) sulphate * Eye Protection Hypothesis: This lab will demonstrate a dehydration reaction. When the beaker containing hydrated copper (II) sulphate is heated, the water will evaporate, causing the color to change from blue to white, and the mass to decrease. Procedure: 1. Measure & record mass of beaker 2.
Chemical Bonding, structure and Quantity Aim To investigating a range of compound which include metallic, covalent molecular, covalent giant and ionic giant Materials used and list of apparatus Google Bunsen burner Test tube Power supply Spatula Tongs Mats Method To discover the characteristic physical properties of the substances six tests were done. These were tests of appearance, melting point, conductivity of solid, solubility in water, conductivity of solution and hardness. Test 1: Appearance. This was to note whether the substance was shiny, dull, with colour etc. Test 2: Melting point.
Diffusion in a liquid * Droppers / Teat pipette * Thistle funnel * SpatulaC. Diffusion in a solid * Stoppers * Test tubes * Test tube rack * Retort stand and clamp | Material | A. Diffusion in a gas * Liquid bromine, Br2B. Diffusion in a liquid * 1 mol dm-3 potassium manganate (VII), KMnO4solution * WaterC. Diffusion in a solid * Potassium manganate(VII), KMnO4 crystal / Copper(II) sulphate, CuSO4 crystal * Hot liquid gel | Variables | * Manipulated variable: Type of medium * Responding variable: Motion of the particles * Controlled / Fixed variable: Temperature and pressure | Number | Activity 2.2 | Pg. | 8 | Title | Rate of diffusion depends on the temperature | Aim | To show that the rate of diffusion depends on the temperature | Problem Statement | How does rate of diffusion depends on the temperature?