How many moles of zinc are in a penny? Purpose: this lab is being performed so students can visualize a single-replacement reaction and calculate how much zinc is in a post-1982 penny? Materials: A post- 1982 penny steel wool 3 M HCl graduated cylinder Small beaker tongs Balance paper towels Sharp edge Safety: 3 M hydrochloric acid (HCl) is fairly caustic. Wash hands immediately is you spill on them. Wear goggles.
Collect 6 grams of copper (II) sulfate on weighing paper. Weigh and record. 5. Collect 50 mL of distilled water into the beaker. 6.
Determining the Percent of Copper and Zinc in Pennies Objective: * Find a way to measure the percent of density of the zinc and copper in pennies * Use best-fit straight line to examine linear relationships, and use it to create a predictive model to determine the percents * Learn to record lab data and observations, and practice with safe procedures in the lab. Background: As we know of today pennies are not made with just copper, they are made with many different metals and have a copper coating. To find the percent of copper you need to find the densities of the materials that make up a penny and then find the mass of just the copper and you can find a percent. Experiment Procedure: Determine the density of the following percentages of Zinc and Copper mixtures. Then compare the precision and accuracy of the data to the literature values for pre and post 1892 pennies when using various numbers of coins.
The purpose of the experiment was to do a solution, which molarity is 0.20 mol/l, from water and an ionic compound. Our ionic compound was zinc sulfate (ZnSO4). Our task was to make one hundred milliliters (100 ml) of the solution. Materials To execute the experiment we used the following equipment: - a beaker - a volumetric flask - a plastic spoon - a scale - a pipette - a funnel - a cork cap We also used solid zinc sulfate (ZnSO4), and distilled and deionized water to make the solution. Calculations To figure out the amount of zinc sulfate that we had to add to the water, so that the molarity of the solution would be 0.20 g/mol, we did the following steps: First we calculated the amount of the zinc sulfate to add in moles.
(b) What accounts for the difference(s)? (c) What specific process is occurring in each container? (d) How do you know when the processes are complete? (e) Use your observations to rank the three elements hydrogen, copper, and zinc from most to least reactive. a) Bubbles stop in the lemon juice first but are still forming in the vinegar.
Hypothesis: Using melting points can help determine the difference in total carbon atoms and branches between two or more compounds. Materials List: 1 Spoon 1 Paper towels 3 Small rubber bands 2 Clean sheets of paper 1 Beaker, 100 mL, glass 1 Burner-fuel 1 Burner-stand 1 Goggles-Safety 1 Magnifier, dual 1 Thermometer-in-cardboard-tube 1 Capillary tubes-3/pack 1 Tetracosane Crystals - 0.2 g in Vial 1 Tetradecanol Crystals - 0.2 g in Vial Procedures: Prior to beginning the lab exercise, read the instructions carefully. Begin by setting up a derivative melting point table to collect the data accumulated during the exercise. This lab uses heated water so be sure to follow safety procedures carefully. While conducting this laboratory experiment, be sure to use minimal amounts of each substance in order to create the habit of using only the amount necessary.
Appearance Iodine: silver sphere solid Zinc Shot: Round flat silver Zinc Granular: pencil shaving like silver solid Potassium iodide: white thick powder Focus Question: How well does the appearance and solubility of iodine and zinc respectively compare with information presented in the CRC Handbook of Chemistry and Physics? The appearance and solubility of iodine and zinc that we observed n the lab are very similar to the information presented in the CRC handbook of chemistry and physics. The iodine pieces we observed in lab were insoluble in water, and soluble in potassium iodide (very soluble), mineral oil (slightly soluble), and alcohol (slightly soluble). This consigns with what the CSC handbook stated that’s potassium iodide,
You now have sao mL of a zinc iodide aqueous solution. On the label of the flask you write (there ca'n be many different possibilities): ( tl ;)'II I ! Exercise 2. Two students need zinc iodide that is in solution in the following amounts: Student 1 : 0.43 g of zinc
Transform the data into the a graph- Cumulative Mass of zinc in grams (y-axis) vs cumulative displaced water in mLs (x-axis) Confidence Report- My partner and I are very confident in our results gathered during is lab. The density of the zinc found during the experiment was 7.0 g/mL. This value is very close to the value stated in the CRC Handbook of Chemistry, which is 7.14 g/mL. As for our materials, the beakers and graduated cylinders where cleaned thoroughly to prevent contamination in our observations of zinc and iodine. The test-tubes used for the solubility tests of zinc and iodine were washed and dried as well.
We’re specifically looking into how much product will be created after conducting experiments with various different concentrations of Iodine and Zinc. One of the things we tested for was the production of a “white solid” which acted as our precipitate. Another key element we kept an eye out for was excess zinc, which showed us how much of the zinc was reacted. During our experiment we colleged exactly the amounts we needed for our group, no decimal point less! We also collected an accurate amount of acidified water, used to start the reaction.