nitrate and potassium iodide solutions Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction. 3. Magnesium metal and hydrochloric acid solution Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next‚ place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas. 4. Electrolysis of water
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Before starting this experiment we were explicably told to have all glassware was dried to insure no water. However water could have still gotten into the reaction and this would react with the Grignard reagent‚ causing a reduction of the phenyl magnesium bromide to the hydrocarbon benzene. This would contaminate our product‚ consequently lowering our melting point. To avoid this contaminate‚ the glassware used was dried and the apparatus was closed with calcium chloride and a cotton ball. During
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mathematical relationships‚ and a balanced chemical equation. Theory: The goal of this lab is to find the volume of one mole of hydrogen at STP. The experimenters will be working with hydrochloric acid and magnesium to find the objective. The acid in this lab will react to the magnesium and cause the water in the eudiometer to rise because of the reaction. The final volume should be 49.92mL.A Key theory to know for this lab is Avogadro’s hypothesis. This statesthat “equal volumes of gases at the
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apparatus and coming out into the atmosphere. After setting this up‚ researchers continued to crush magnesium turnings into smaller pieces in order to expose fresh metal by removing possible magnesium oxide that was on the surface of the turnings. The turnings were added to the round bottom flask as well as an iodine crystal‚ which facilitates the reaction by cleaning the surface of the magnesium metal. Bromobenzene and anhydrous diethyl ether were then added to the flask. Anhydrous ether was used
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Table 8.1- Combustion of magnesium ribbon Observations Reaction was exothermic; magnesium ribbon burned and was glowing a bright white color when ignited. Reactants: Mg and O2 Products: MgO Balanced chemical equation 2Mg + O2 2MgO Table 8.2- Combustion of heptane Observations When holding test tube inverted over heptane flame‚ condensation formed against top walls of the test tube. When the burning splint was added the walls of the test tube became less foggy from the condensation
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experiment and graphs – PG 7+ Chemistry coursework Hypothesis/Aims The aim of the investigation is to see how different concentrations of hydrochloric acid affects the rate at which hydrogen gas is produced when it’s reacted with a strip of magnesium. The rate of reaction is a measure of change that happens in a single unit of time. When a reaction takes place the particles of the reactants collide. The more often the particles collide the more likely they are to react and so the faster the
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its effective surface area is much the same as (or even less than) it would be if it were present in a single lump. A small heap of fine magnesium powder tends to burn rather more slowly than a strip of magnesium ribbon‚ for example. Imagine a reaction between magnesium metal and a dilute acid like hydrochloric acid. The reaction involves collision between magnesium atoms and hydrogen ions. How does surface area affect a chemical reaction? If one of the reactants is a solid‚ the surface area of the
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reaction‚ thus‚ of a chemical change. Materials Crucible tongs Evaporating dish Glass rod Test tubes Test tube rack Thermometer Analytical balance Magnesium ribbon pH paper 1M copper (II) sulfate Iron metal 6M hydrochloric acid Procedure Magnesium and oxygen test A small strip of magnesium metal is held on one end with a pair of crucible tongs‚ while the other end is ignited with the flame of Bunsen burner. The burning ribbon is held over a clean evaporating
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Locker# 1137 Date of Experiment: May 11‚ 2014 Date of Submission: May 16‚ 2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass (g) Crucible + Lid 30.581g Crucible + Lid + Hydrated compound 31.590g Hydrated Compound 1.004g
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NSS Chemistry Part 3 Metals HKCEE Past Paper Questions – Structural Questions 1. HKCEE 1995 Q1 Rubidium (Rb) and potassium belong to the same group in the Periodic Table. The relative atomic mass of rubidium is larger then that of potassium. (a) Explain whether rubidium is more reactive than potassium. (b) Write a chemical equation for the reaction between rubidium and water. (State symbols should be given.) (c) Suggest how rubidium can be stored safely in the laboratory.
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