moles in 2.65g of zinc. 2. Calculate the number of moles of hydrochloric acid in 37.5mL of a 3.00M HCl solution. 3. Calculate how many moles of HCl are required to react with 0.244 moles of zinc. Procedure: 1. Put on safety equipment. 2. Label small glass vial so your group can identify it later. 3. Determine the mass of the clean dry vial and record your mass to 2 decimal places on your lab sheet. 4. Zero the balance. 5. Add 3-4 grams of zinc to the vial and
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mm) 4 beakers (150 mL) Safety goggles Lab apron Plastic gloves Full face shield Reagents Zinc Magnesium Iron Copper 1M hydrochloric acid‚ HCl 1M sulphuric acid‚ H2SO4 1M acetic acid‚ HC2H3O2 1M phosphoric acid‚ H3PO4 Procedure: Please refer to Health Chemistry‚ Laboratory Experiments‚ page(s) 75-76. Data and Observations: Table 1: Comparison of Metal Activities Zinc Magnesium Copper Iron Hydrochloric acid Small bubbles Many bubbles N.R. color change (black)
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Abstract This lab is performed in order to determine the total energy in a reaction between zinc and hydrochloric acid. The reaction is done twice‚ once to measure the heat of the reaction and again to determine the work done in the system. This is because Enthalpy equals heat plus work (∆H= ∆E+W). Heat and work can be broken down further into separate components so the equation used in lab is ∆H=mc∆T + PV. Many calculations are used in the lab to find out what cannot be measured directly (ex:
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Effect of Particle Size solid zinc‚ approx. 0.5 cm × 2 cm‚ or solid marble chips zinc powder or calcium carbonate powder balance 2 test tubes 1M HCl (approx 10 mL per group) Part 2. Effect of Temperature 3 Alka Seltzer tablets 3 250-mL beakers water at three temperatures – with ice‚ room temperature‚ warm (around 70°C) Part 3. Effect of Concentration 1M HCl‚ 5 mL per group 3M HCl‚ 5 mL per group 6M HCl‚ 5 mL per group 3 pieces of zinc metal‚ each approx 1 cm × 1 cm 3 test
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Percent Composition of a Penny Background 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
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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 of red litmus paper and record observations. 3. Place a drop
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experiment will be using HCl a strong acid to dissolve all the zinc inside the outer copper shell. The reaction follows as such; Zn+2HCLZnCl2+H2‚ but there will be no reaction with copper. The portion that will be measured is the mass of copper left after all of the Zn goes through the reaction process. Hypothesis: If the penny is post-1983‚ then there will be a percent yield of copper greater than 30%. Research Question: What is the percent composition of Copper and Zinc in a post-1983 penny?
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Chemical Equilibrium: Le Chatelier Principle By Sarah Ramos and Kristina Todorovic Chemistry 203 DEN Dr. Mohamed El-Maazawi Part A. Acid-Base Indicators Purpose In this part of the experiment‚ we will find a reagent that will shift the acid-base equilibrium reaction described by Equation (2) in one direction and then a second reagent that will cause the equilibrium position to shift back in the opposite direction. Introduction An acid–base indicator
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Observation Zinc Shot: Silver color‚ some pieces are shiny while the majority is dull. Tear shaped pieces (round at base with pointed top). No odor. Zinc Granular: Silver in color‚ semi shiny‚ flaky appearance. No odor. Zinc Sheet: Sheet of metal‚ flat pieces that are about 3 inches wide & 2 inches in length & 0.02 inches in height. Each piece has a dull side and a shiny side. Silver in color‚ the dull side has a darker shade of gray. No odor. Zinc Powder: Gray very fine powder. No odor
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EXPERIMENT-1 CHEMICAL REACTIONS AIM: To perform and observe the following reactions and classify them into: (i) Combination reaction (action of water on quick lime) (ii) Decomposition reaction (action of heat on ferrous sulphate crystals) (iii) Displacement reaction (iron nails kept in copper sulphate solution) (vi)Double decomposition reaction (reaction between sodium sulphate and barium chloride) APPARATUS REQUIRED: 1. A rack of at least six clean test tubes and a boiling
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