wk 3 lab document

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Baker College, Auburn Hills *

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120

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Chemistry

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May 25, 2024

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docx

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OL Lab 3: Stoichiometry: Avogadro’s number and molecular calculations / Solution Preparation: From salt to solution Learning Objectives:  Explain the relationship between mass, molecular weight, and numbers of atoms or molecules and perform calculations deriving these quantities from one another  Perform mass-to-mass stoichiometric calculations via conversions to moles  Identify the limiting and excess reagents in a chemical reaction  Calculate the theoretical, actual and percent reaction yield  Define Avogadro’s number and describe the mole quantification of matter  Explain relationship between mass, molecular weight, and numbers of atoms or molecules  Perform conversion and derivations calculations using key molecular quantity parameters  Define Avogadro’s number and describe the mole quantification of matter How many moles of sand grains has the Sahara desert? What is the only equation you ´ll ever need in chemistry? The short stoichiometry simulation will help you answer those questions! Follow the footsteps of great chemists and learn about key molecular parameters based on one and only star of chemistry calculations: Avogadro’s Law! Concept mole and Avogadro’s Law: Your first mission in this short simulation is to familiarize yourself with the concept of mole and the way of counting molecules of substances using the one and only Avogadro’s Law. You will learn how to convert huge numbers of particles into handy Avogadro’s number, extensively used by all chemists around the world! Chemical units relationship: Next, you will explore the relationship between mass, molecular weight, and number of atoms. This magical equation will enable you to perform derivations of molecular quantity parameters for various chemical substances. You will feel like Marie Curie analysing chemical dependencies of chemicals in her French laboratory! Part 1: Complete the Labster lab: Stoichiometric calculations: Identify an unknown compound using gravimetric analysis. Glassware and quantitative transfer Moving on to the second workbench, you will explore and determine what glassware will be appropriate for you to use. Your lab guide and mentor, Dr. One, will walk you through the process of preparing the solution. You will have the freedom to use the equipment as you like, but only by following Dr. One’s instructions will you be successful in making the right solution. To make sure you can always redo the essential steps of the process,

Dr. One will provide you with a fantastic reset button, so you can try again if you make a mistake. Solve the preparation In the end, only by carefully ensuring that the right amount of water and ammonium chloride is used can you make the correct solution. Are you prepared for solving how to perform a Solution Preparation? Part 1: Complete the Labster Lab: Stoichiometry: Avogadro’s number and molecular calculations Complete all activities and answer all questions within the lab and then complete the questions below: Purpose: Describe in complete sentences and in your own words, the purpose of this experiment. This experiment was designed to introduce Avogadro's number and demonstrate how atoms may be counted using it. Observations: Record three observations from the simulation. I. The number of atoms in a substance is called a mole. II. The number of molecules in an iron screw, a glass of water, and Saharan sand is the same . III. Determing the molar mass can be found by using this equaton: M(G/mol)= mass(grams) /n(moles) 1. How do you convert between grams and moles of a specific molecule? Give a specific example to illustrate. Calculate the material molecule's mass in grams. Use the Periodic Table to calculate the substance's molar mass (also known as its relative formula mass).Utilizing the formula, determine how many moles of the material there are. Moles= mass in grams/molar mass 2. How do you convert between moles of one substance and moles another substance? The mole ratio determined from the balanced chemical equation can be used to convert between moles of one material and moles of another. In the balanced equation, the coefficients indicate the relationship between the substances.

3. Balance the following chemical equation: Na 2 CO 3 (aq) + CaCl 2 (aq) → CaCO 3 (s) + NaCl(aq) We need two Na and two Cl on the products to equal the reactants in order to balance since Ca and CO are equal for both the reactants and the products. Consequently, Na = 1 x 2 = 2 and Cl = 1 x 2 = 2 Therefore, CaCO 3(s)+2NaCl(aq) will be the balanced products. Moreover, Na 2CO3(aq)+CaCl 2(aq)→CaCO 3(s)+2NaCl(aq) is the balanced equation. 4. Use the balanced chemical equation from the last question to solve this situation: You combine 0.5 moles of Na 2 CO 3 with enough CaCl 2 that your compound reacts completely. How many moles of NaCl would you expect this reaction to produce? Show all work below. If you are not sure how to complete this problem, please see the video here: https://care.mediaspace.kaltura.com/playlist/dedicated/254042593/1_aw4f9v30/1_4 xqaj516 One mole of Na2CO3 and one mole of CaCl2 react to form one mole of CaCO3 and two moles of NaCl, as can be shown from the balancing equation. Consequently, you would anticipate producing 0.5 * 2 = 1 mole of NaCl if you start with 0.5 moles of Na2CO3 and adequate CaCl2. Part 2: Complete the Labster Lab: Solution Preparation: From salt to solution Complete all activities and answer all questions within the lab and then complete the questions below: 1. In this lab, you learned how to prepare solutions with a precise concentration. Where in your nursing career might this skill be needed? If you work in a medical-surgical facility, you might need to combine insulin, antibiotics, or any other kind of prescription drug on a daily basis. Knowing which IV drip medications can be hung together before hanging and what to look for if not is crucial . 2. Which piece of glassware did you use to prepare your solution in this lab and why? I choose to use a volumetric flask because it is a highly accurate and suitable glassware type for combining various chemicals. 3. Calculate how many grams of NaCl are required to make 100 mL of a 1 M NaCl solution. Show your work in the space below.

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