Litmus paper • Pipets • Spatula • Test tubes Materials: Ammonium carbonate‚ 0.5g Calcium carbonate‚ 0.5g Copper chloride solution‚ 4mL Hydrochloric acid‚ 4mL Magnesium ribbon‚ 2-4 cm strips Phenolphthalein indicator‚ 1 drop Sodium hydroxide solution‚ 1mL Sodium phosphate solution‚ 1mL Water Zinc‚ mossy‚ or zinc shot‚ 1-2 pieces Introduction: In this lab we will classify different chemical reactions. Classifying chemical reactions allows us to predict what chemical
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64 65 75 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton 24 96 25 31 115 32 119 33 122 34 128 35 127 36
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equations Part I: Reaction between zinc and iodine Watch the Video. http://www.youtube.com/watch?v=xT9V7Y1iKYc Observations: Describe what happened when the water was added. A reaction happened and the iodine exploded into a purple gas Questions and conclusions: 1. Balance the equation‚ if necessary‚ for the reaction between zinc and iodine. Zn + I2 ZnI2 It is balanced 2. Classify the reaction that occurred between the zinc and iodine. redox 3. What evidence
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experiment conducted‚ the three metals‚ magnesium‚ zinc and copper each had to undergo displacement reactions and reactions with water‚ oxygen and dilute acids‚ to arrange them in the order of their reactivity. Generally‚ the more easily a metal burns in air to form an oxide‚ the higher up it is in the reactivity series. It was observed that both zinc and magnesium burned in air to form their corresponding metal oxides (magnesium oxide and zinc oxide) but copper did not undergo any such reaction
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calcium sulfide. Δ Ca (s) + S (s) → CaS (s) b. Hydrogen gas reacts with fluorine gas to produce hydrogen fluoride gas. H2 (g) + F2 (g) → 2 HF(g) c. Solid aluminum metal reacts with aqueous zinc chloride to produce solid zinc metal and aluminum chloride. (Check the Solubility Rules to determine the phase of matter of aluminum chloride.) 2 Al (s) + 3 ZnCl2 (aq) → 2 Zn (s) + 2 AlCl3 (aq) 4. Translate the following chemical equations
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reactivity series. Materials : * Hydrochloric acid (1M) * Metals (sodium‚ calcium‚ magnesium‚ aluminium‚ zinc‚ iron‚ tin‚ lead‚ copper) * 9 test tubes * Test tube rack * Test tube holder * Retort stand * Bunsen burner * Beaker * Tripod * Heat proof board * Wire mesh * Water Methods: Acid and Metal * Using a carving knife/cutter‚ cut out a piece of metal weighing 1g. * In each test tube‚ pour in 2ml of Hydrochloric acid per test tube. * Add
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The reactivity series is the known series of how metals should react. It places Calcium as the most reactive (of the metals being tested in this experiment)‚ followed by Magnesium‚ Aluminium‚ Zinc‚ Iron‚ Tin and finally‚ as the least reactive (of the metals being tested in this experiment)‚ Copper. However‚ the results this experiment produced did not follow this trend. If the metal that produces the most hydrogen gas is considered the most reactive‚ in this experiment magnesium was most reactive
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rusting No reaction Table 2: Observations Results: HCl(Solution used) Metal Word Equation Balanced Equation Cu NR NR Mg Magnesium + Hydrochloric Acid ---> Hydrogen + Magnesium Chloride Mg(s) + 2HCl(aq) ---> H2(g) + MgCl2(s) Sn NR NR Zn NR NR Fe NR NR Steel (FeAl) Iron (III) + Hydrochloric Acid ---> Hydrogen + Iron (III) Chloride 2Fe(s) + 6HCl(aq) ---> 3H2(g) + 2FeCl3(s)
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Writing Complete Equations Practice For each of the following problems‚ write complete chemical equations to describe the chemical process taking place. Important note: There are a few physical processes on this sheet – You can’t write an equation for a physical process! 1) When lithium hydroxide pellets are added to a solution of sulfuric acid (dihydrogen sulfate)‚ lithium sulfate and water are formed. 2) When dirty water is boiled for purification purposes‚ the temperature is brought up to
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beaker with tongs off of the hotplate and filtered the solution with a filter paper and funnel. The next day‚ after the solid had dried onto the filter paper‚ we scraped the solid off and into the beaker with a spatula. We then added sulfuric acid and zinc‚ respectively‚ into the beaker. We stirred the solution and our final step was getting rid of the liquid waste and observing the copper powder at the bottom of our beakers. We noticed that although we performed many different chemical reactions
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