LR lab Marlena Slade

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School

Massachusetts Bay Community College *

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Course

101

Subject

Chemistry

Date

Jan 9, 2024

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pdf

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Uploaded by ConstableStrawScorpion146

Limiting Reagent Lab

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Introduction: In a chemical reaction, the limiting reagent is the reactant that is totally consumed when the chemical reaction is completed, and it determines the quantity of the products that are produced. The other reactants present in the reactions are sometimes found to be in excess since there is some leftover quantity of them after the limiting reagent is completely used up. The maximum amount of product that is produced is known as the theoretical yield. The limiting reagent should be identified to calculate the percentage yield of a reaction. The purpose of this lab is to find the limiting reactant in a chemical reaction. The question is, how do you find the limiting reactant in a chemical reaction in the simplest way? Experiment Objectives ● Apply dimensional analysis and the concept of limiting reactants in an example about baking cookies ● Investigate a chemical reaction involving aluminum metal and copper(II) chloride dihydrate ● Use observations before and after and stoichiometry to determine a limiting reactant ● Calculate theoretical yields and the percent yield. Safety Considerations ● Wear your safety goggles at all times during the experiment. ● Sulfuric acid is a strong acid and is corrosive to skin and eyes and toxic to inhale. Handle H 2 SO 4 solutions carefully. ● Read the label of the chemical before using. Experimental Procedure This week, we will work with copper and aluminum. As an element, copper is a shiny brown metal (like a penny) whose surface will slowly change color to bluish/green (like the statue of Liberty). As an element, aluminum is a shiny silvery metal. Its surface also reacts, but without the dramatic color change. The reaction we will perform today is between aluminum metal + copper(II) chloride dihydrate solution.

You will need the balanced chemical equation for the reaction to be able to analyze your results. You should be able to figure out the products from your observations. You must watch the following video, follow the procedure, and record the data. https://www.youtube.com/watch?v=xDjhHES9HnE 1. Weigh a filter paper and record its mass. 2. Using the same analytical balance (it's good practice to use the same balance during an experiment to minimize uncertainty), weigh the Aluminum foil and record the exact mass. 3. Weigh your copper(II) chloride dihydrate solid in a small beaker and record the mass. 4. Dissolve the copper(II) chloride dihydrate in water and record its color. 5. Place the Al foil in the beaker containing copper(II) chloride dihydrate solution and add 1-2 drops of sulfuric acid. 6. Stir the substances in the beakers occasionally with the stirring rod and break up the aluminum foil as it reacts. The reaction should take about 30 minutes to complete. 7. Record any color changes or any other observations during the reaction. 8. Allow the solid copper to settle in the beaker. Filter out the solution from the beaker using the filter paper. 9. Wash the copper metal in the filter paper with 15 mL of deionized water. 10.Use an oven and dry out the filter paper. 11. When the product appears dry, carefully place the filter paper on paper towels. 12.After cooling, weigh the filter paper. Record this in your data table. Data: 1. Mass of the filter paper= 1.49g 2. Mass of Al foil=0.60g 3. Mass of copper(II) chloride dihydrate=6.35g

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4. Molar mass of copper(II) chloride dihydrate=170.69 g/mol 5. Mass of copper metal recovered + filter paper= 3.38 g Questions and calculations: 1. Write the formula of copper(II) chloride dihydrate. cucl2 2H2O 2. What is the molar mass of copper(II) chloride dihydrate? 170.49 g/mol 3. Write the balanced chemical equation for the lab. Make sure to include the state of each reactant and product. 4. What is the color of copper(II) chloride dihydrate solution? 5. Write your observation including the color change during the reaction. 6. Identify the reaction. 7. Would you be able to determine the Limiting Reagent by just observing the reaction? Why or why not?

8. Calculate the moles of Al foil. Show your work for credit. Use proper DA, units, and SF. 9. Calculate the moles of copper(II) chloride dihydrate. Show your work for credit. Use proper DA, units, and SF. 10.Determine the LR. Do not just name it, show your work. Use proper DA, units, and SF. 11. Calculate the theoretical yield of Cu metal in grams. Show your work for credit. Use proper DA, units, and SF. 12.Calculate the experimental yield of copper. Show your work for credit. Use proper DA, units, and SF. 13.What is the %Yield of copper? Show your work for credit. Use proper DA, units, and SF.

14.Explain the rule of sulfuric acid in this reaction. Post-Lab Questions 1. Si 3 N 4 is made by combining Si and nitrogen gas at a high temperature. How grams of Si 3 N 4 are produced by reacting 2.3 moles of Si and 2.3 moles of nitrogen gas? Write the balanced equation and show your work. Use proper DA, units, and SF. 2. What would be the experimental yield of Si 3 N 4 if the percent yield of the reaction is 95% in the above question? 3. Identify the reaction in question 1. 4. In the following reaction: 4NH 3 (g) + 5O 2 (g) → 4NO (g) + 6H 2 O (l)

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When 2.2 moles of ammonia and 2.4 moles of O 2 are mixed, then the mass of water formed will be_____________. Identify the LR by showing your work. Use proper DA, units, and SF.

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