of layers of zinc atoms around a piece of galvanized iron. This was done by pouring the hydrochloric acid onto the galvanized iron‚ thus removing the zinc from the piece of metal. Laboratory Procedure 1. Measured and recorded the mass of a piece of galvanized iron using a centigram balance and a ruler 2. Measured and recorded the length and width of the galvanized iron using the ruler 3. Put the piece galvanized iron into a 400-ml beaker 4. Added 25mL of hydrochloric acid to the
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CHANGE IN MASS(±0.005g) OF VARIOUS TYPES OF CORROSIVE METALS WHEN PLACED IN A SOLUTION OF 1 MOLAR CONCENTRATION OF HYDROCHLORIC ACID OVER A PERIOD OF 8 DAYS AT AN AVERGAE ROOM TEMPERATUR OF 24 DEGRESS CELCIUS. Research Question: Does the mass(±0.005g) of various types of corrosive metals (iron‚ nickel‚ zinc‚ copper and tin) change when placed in a solution of 1 molar hydrochloric acid over a period of 8 days at an average room temperature of 24 degrees Celsius? Aim: To be able to record and understand
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displace Iron because it is more reactive. Zinc + Hydrochloric acid: Zinc will replace Hydrogen because it is more reactive. Copper + Hydrochloric Acid: Copper will not displace Hydrogen because copper is more reactive. Magnesium + Hydrochloric acid: Magnesium will displace Hydrogen because it is more reactive and end up as Magnesium Chloride + Hydrogen. Sodium + Hydrochloric acid: Sodium will displace Hydrogen because
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Schmoe Period 3 March 8‚ 2013 Lab Report: Empirical Formula of Zinc Chloride (ZnCl) * Purpose The purpose of this experiment was to learn how to determine the empirical formula. Empirical means “based on experimental evidence.” * Experimental Design The reaction that occurred was the reaction of the elements Zinc (Zn) and Chloride (Cl) by mixing a piece(s) of Zinc and 50mL of Hydrochloric Acid (HCl). The amount of Zinc was determined to be between 1.00g and 1.25g. As the reaction occurred
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Information: Post-1983 pennies have a copper jacket and a zinc core. We hope to determine the percent composition of these two metals. This will be done by reacting the zinc with hydrochloric acid to form zinc ions in a single replacement reaction. The acid reacts with the zinc but not copper. The reaction of zinc metal with the hydrochloric acid (HCl) produces zinc chloride and hydrogen gas. Safety: Wear your safety goggles and apron If you spill Hydrochloric acid on yourself‚ rinse with water Procedure: DAY
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Making and Testing for Hydrogen Gas Felicity Tyler Aim: To produce and test for hydrogen gas. Materials: * rubber stopper * dilute hydrochloric acid (HCI) * zinc pieces (Zn) * test-tube rack * matches * dilute sulphuric acid (H2SO4) * 2 cm strips of magnesium ribbon (Mg) * Iron pieces (Fe) * Test-tube Method 1. Test the different metals with the acids by separately combining
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tubes and rack • Test tube holder • Bunsen burner • Hydrochloric acid 0.1M • Copper sulphate solution 0.5M • Bunsen burner Method Diagrams of the set up for experiments: 1‚ 2 and 3 Experiment 1 1. Pour about 1cm of hydrochloric acid into each test tube 2. Drop a piece of zinc into each of the first two test tubes. Reduce the concentration of the hydrochloric acid in the second test tube by adding water until it is half-full.
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equipment: X 12 test tubes X 10-mL graduated cylinder X Water ¡V deionizer (distilled water) X 0.1M cobalt (II) chloride hexahydrate X 95% ethanol X 0.1M cobalt (II) chloride hexahydrate dissolved in 95% ethanol X zinc X 1M hydrochloric acid solution X 0.1M copper (II) sulfate solution X 0.5M sodium hydrogen carbonate solution X 1M ammonia solution X magnesium X 1M sodium hydroxide solution X ammonium chloride Procedure: A. Be sure to always
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the different reactions formed between various acids and bases with the aid of indicators. Equipment: 1. Safety goggles. 2. Droppers. 3. Red Litmus paper. 4. Blue Litmus paper. 5. pH paper. 6. Well plate. 7. Micro spatula. Materials: 1. Zinc. 2. Magnesium. 3. Iron. 4. Copper. 5. HCL. 6. HC₂H₃O₂. 7. NaOH. 8. Phenolphthalein. Procedure: Part A: 1. Add five drops of HCL‚ HC₂H₃O₂‚ and NaOH to different depressions in the well plate. 2. Place a drop of each solution onto a piece
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During the first step of this lab‚ when obtaining the hydrogen from the mossy zinc and the hydrochloric acid‚ it took a lot longer than I thought it would for the water in the pipet to be displaced. I was tempted to remove the stopper and add another piece of zinc and see if that would make it go faster‚ but I did not want to interrupt the process. It seemed the longer that the mossy zinc was exposed to the hydrochloric acid the faster it dissolved and therefore more gas was produced. When the manganese
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