OL Lab 3_ Stoichiometry_ Avogadro’s number and molecular calculations _ Solution Preparation_ From s

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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. In this experiment, we aim to explore stoichiometric calculations and the art of balancing equations. The goal is to dive into the relationships between mass, molecular weight, and the numbers of atoms or molecules. Through these experiments, we'll practice deriving these quantities from one another, gaining a better understanding of the intricate connections within chemical reactions. Observations: Record three observations from the simulation. I. Balancing equations is like the stabilizer for keeping the mass in check in a chemical equation. It's the trick that ensures everything adds up nicely. II. A glass of water actually contains more water molecules than there are grains of sand in the entire Sahara Desert. III. Avogadro's number comes in handy when we're dealing with large quantities, which is pretty common when we're talking about atoms and molecules. It's like our go-to tool for handling those big numbers in the realm of tiny particles. 1. How do you convert between grams and moles of a specific molecule? Give a specific example to illustrate. First things first, you begin by multiplying the number of atoms by the atomic weight for each element in the compound. After that, you sum up all your answers to get what we call the molar mass. And finally, to wrap it up, you divide the number of grams of the compound by the molar mass to figure out the number of moles. 1. How do you convert between moles of one substance and moles another substance? If you want to switch from one mass (let's call it substance A) to another mass (substance B), the process goes like this: first, transform the mass of A into moles, then apply the mole-to-mole conversion factor (B/A), and finally, convert the mole quantity of B back into grams of B. It's like a step-by-step dance to get from A to B. 1. Balance the following chemical equation: Na 2 CO 3 (aq) + CaCl 2 (aq) → CaCO 3 (s) + NaCl(aq)

Taking a quick look at the equation, you'll see that everything matches up on both sides, except for Na and Cl. To fix this, we just need to tweak the coefficient on the right side and make it 2NaCl. So, the balanced equation would look like this: Na2CO3(aq) + CaCl2(aq) → CaCO3(s) + 2NaCl(aq) 1. 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 _4xqaj516 Na2CO3 + CaCl2 → 2NaCl + CaCO3 106g of Na2CO3 - 1 mole 0.5g of Na2CO3 = 0.5 ÷ 106 = 0.0047 moles. 1 mole of NaCl - 58.5 0.0047 moles = 0.0047 × 58.5 = 0.27g. 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? The meticulousness required in preparing solutions feels a lot like handling patient medications. Just like when administering medications intravenously, precision is key — it's crucial to be 100% accurate and exercise extreme caution. The skills honed in chemistry will undoubtedly contribute to maintaining accuracy when delivering these medications in my future work. 1. Which piece of glassware did you use to prepare your solution in this lab and why? We used a volumetric flask to prepare the solution. The size of the flask at the top is narrow, and can sometimes make it difficult to add solids or powders to the flask. In this case it provided the most accurate reading on the amount of liquid we added to the powder, which gave us the advantage of being twice as accurate as a traditional beaker. The narrow top also allowed us to mix the solution easily.

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