Calcuate the empirical formula of magnesium oxide. The experiment can be improved - can you suggest how? Music: "twine and timber" by Russianhush on sound cloud Sound effect from half life (Valve) and mickmon from freesound.org
Views: 2313 Richard Thornley
calculations and conclusions on finishing the empirical formula lab.
Views: 11767 turdfurg67
This is a detailed video on how you could determine the empirical formula of a compound using experimental data. This video is super helpful in understanding our next topic on determining the empirical and molecular formulas of compounds from mass data.
Views: 2080 Anthony Tedaldi
This chemistry video tutorial explains how to find the empirical formula given the mass in grams or from the percent composition of each element in a compound. If you're given the mass percent, you can simply treat it as if you were given the mass in grams. This video explains how to find the molecular formula given the molar mass of the compound. You can do this once you have the empirical formula. This video explains all of it. It has plenty of practice problems and examples for you to master this lesson. New Chemistry Video Playlist: https://www.youtube.com/watch?v=bka20Q9TN6M&t=25s&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS&index=1 Access to Premium Videos: https://www.patreon.com/MathScienceTutor
Views: 197133 The Organic Chemistry Tutor
Empirical Formulas - It starts with the percent composition of a compound, explains what empirical formula is, and uses a table to organize the various steps. http://www.BCLearningNetwork.com. 0:00in this example will learn what an 0:02empirical formula is how we can find it 0:05given the percent NASA's of elements in 0:07a compound and organic compounds 0:09analyzed by a mass spectrometer and 0:12found to be 39.2 33 percent carbon 1.82 0:179% hydrogen 38.6 03 percent chlorine and 0:2320.3 three five percent nitrogen by mass 0:26determine the empirical formula for this 0:29compound now what exactly is an 0:32empirical formula let's look at an 0:35example of a different compound let's 0:37say the molecular formula for a compound 0:40is sea tan h6 cl8 the molecular formula 0:44tells us how many atoms of each element 0:46are in one molecule of this compound so 0:50one molecule has 10 c atoms 6 h atoms 0:54and HCL Adams the empirical formula 0:57gives a smallest whole number ratio of 1:00Adams taking a look at the molecular 1:02formula c 10 h 6 cl8 the subscript 10 6 1:08and 8 are all divisible by 2 so we write 1:12a new formula in which all the 1:14subscripts have been divided by two 1:16which is c 5 h 3 CL for this is called 1:22the empirical formula and it gives the 1:24smallest whole number ratio of atoms the 1:2753 in the four cannot be reduced any 1:30further and it means for every 5 c atoms 1:34there are 3 h atoms and 4-cl atoms so 1:38the empirical formula tells us there are 1:40five see Adams 23 h atoms to 4-cl atoms 1:44of course single atoms are too small 1:46account individually but moles of atoms 1:49or something we can actually measure and 1:51compare in the lab since the mold of any 1:54entity is the same number 1:56it follows that there are five moles of 1:58C Adams 2 3 moles of h atoms for moles 2:02of cl Adams starting with the massive 2:05Beach element in a given sample of a 2:07compound we can find the ratio of moles 2:09of each kind of atom 2:11and therefore the empirical formula now 2:15in this example here were given the 2:17percent mouse's developments rather than 2:19the actual mouse's however all we need 2:21to do is pretend we have a hundred grab 2:23sample and a hundred gram sample 39.2 33 2:28percent of the hundred grams is carbon 2:30so that would mean there are 39.2 33 2:33grams of carbon similarity 1.82 nine 2:37percent of the hundred rounds is 2:39hydrogen so that would mean there at one 2:41point eight to nine grams of hydrogen 2:43and the grounds of chlorine and nitrogen 2:46are also equal to their percent masses 2:48so the original statement of the problem 2:50where percent masses are given can be 2:53changed so that percent masses are 2:55simply changed grams like this here we 3:00can organize our calculations in a handy 3:02table it has six columns something like 3:05this since we have four elements will 3:07make five rows in the first column we 3:10write the symbol for each element in the 3:13second column we know the mass of each 3:15element in the third column we convert 3:18mass in grams to moles of atoms in order 3:21to find the simplest ratio we divide the 3:24moles about him to each element by the 3:26smallest number of moles this we do in 3:28the fourth column we leave a blank in 3:31the fifth column and write the whole 3:32number ratio in the sixth column now 3:36let's use this to carry out our example 3:38the first element is carbon and its mass 3:42is 39.2 33 ground the next element is 3:47hydrogen which has a mass of 1.8 29 3:50grams then chlorine with a massive 38.6 3:5303 grams and finally nitrogen with a 3:57massive 20.3 35 grounds now to calculate 4:01the moles of atoms of carbon we take the 4:04grounds of carbon and x the conversion 4:07factor 1 mole of c atoms 212 grams 4:10notice we write the atomic mass of 4:13carbon by the grabs this gives us 3.27 4:17moles of carbon atoms 4:19we do a similar calculation for hydrogen 4:21we take one point eight to nine grams 4:23and x the conversion factor 1 mole of h 4:27atoms per one ground it's important to 4:30remember we use atomic mass of H not the 4:33molar mass of h2 here when calculating 4:37moles of atoms we always use atomic mass 4:39the atomic mass of hydrogen is 1.0 grams 4:43per mole 4:44this gives us 1.83 moles of hydrogen 4:47atoms to two decimal places for chlorine 4:50we take 38.6 03 ground and since the 4:54atomic mass of chlorine is 35.5 we 4:58multiply by the conversion factor 1 mole 5:0035.5 grams we get 1.09 moles of chlorine
Views: 2655 W CLN
This video is about the AP Chemistry Laboratory - Experiment #9: The Determination of the Formula Mass of an Acid Salt. In this video you will learn how to determine the formula mass of a Potassium acid salt through titration analysis. Students studying Chemistry at different levels could highly benefit from this video.
Views: 1760 Ali Hayek
This video is about the AP Chemistry Laboratory - Experiment #9: The Determination of the Formula Mass of an Acid Salt - within the first year of college program.
Views: 671 Ali Hayek
This chemistry video tutorial focuses on molarity and dilution problems. It shows you how to convert between molarity, grams, moles, and liters. It's very useful for students learning solution stoichiometry. This video contains plenty of notes, examples, equations / formulas and practice problems. Here is a list of topics: 1. How to calculate the Molarity of the solution given grams, moles, volume in ml or liters. 2. Determining the mass given the concentration in molarity and the volume in milliliters. 3. Using unit conversion / dimensional analysis to calculate the volume of the solution in mL. 4. Solute, Solvent, Solution Relationship 5. How to increase and decrease the concentration of a solution by adding water or removing water through dilution or evaporation. 6. Molarity and Dilution Problems - M1V1=M2V2 7. Solution Stoichiometry - Actual Yield, Theoretical Yield, and Percent Yield 8. Molarity Stoichiometry - Limiting and Excess Reactant 9. How To Find The Amount of Excess Reactant Remaining / Left Over in Volume in mL, Mass in grams, and moles 10. Single Replacement Reactions - Metal and Halide Displacement - Activity Series 11. Predicting the products of a double replacement reaction - acid base neutralization and precipitation reactions 12. How to calculate the maximum amount of product / theoretical yield given molarity, volume, and grams of the reactants 13. Basic Dilution Calculations 14. Using the Dilution Formula / Equation M1V1=M2V2 to solve acid base titration problems and redox reaction titrations 15. Mixture Problems - Finding the Molarity after mixing two or more solutions
Views: 174354 The Organic Chemistry Tutor
EMPIRICAL FORMULA OF MAGNESIUM OXIDE الصيفة الاولية لاوكسيد المغنيسيوم خطوات العمل المذكوره في الفيديو مختصره وهذه الخطوات الكاملة PROCEDURE Safety notes: Safety goggles must be worn at all times. If the magnesium flashes during heating, do not look directly at the bright light emitted (it could damage your eyes). 1. Clean a crucible and lid, rinsing thoroughly with deionized water as a last step. 2. Place the clean and dry crucible and cover on a clay triangle and heat strongly for 5 minutes, to drive off any volatile material. 3. While the crucible is heating, weigh approximately 0.3 grams of Mg. 4. Using crucible tongs remove the crucible and cover from the clay triangle and place them on wire gauze to cool. 5. Allow the crucible to cool and weigh the crucible. Handle the crucible with tongs, so you do not leave any deposits from your fingers. Record the weight. 6. Place Mg ribbons on the bottom of the crucible. Then, weigh the crucible with The Mg ribbons inside. Record the weight. 7. Place the cover on the crucible. Heat the crucible gently for 5 minutes. While using the tongs to lift the cover slightly every 30 sec. to admit air. Should the Mg start glowing brightly when the cover is lifted, quickly cover the crucible, remove the bunsen burner, and wait one minute before continuing to heat. 8. Heat the covered crucible strongly for 15 minutes. (Lifting the cover occasionally). 9. Lift the cover to determine whether the ribbon has become a whitish ash. If the ribbon still has its original color, reheat for 10 minutes. Repeat step 9 until the ribbon has become a whitish ash then, allow the crucible to cool. 10. Add 10 drops of deionized water to the product in order to hydrolyze any Mg3N2 biproduct. 11. Partially cover the crucible (leave a slight crack) and heat gently for 2 minutes, then strongly for 10 minutes. Allow the crucible to cool to room temperature. 12. Weigh the crucible and the product. 13. Reheat strongly (5-10 minutes), cool and weigh. Repeat this process until the mass of the cooled end product is constant to within ± 0.2 g. *Do not dispose of your sample until your instructor approves your calculation of the empirical formula * DISPOSAL: Dispose the product in the waste container labeled "waste magnesium oxide” From the weights you have collected, you should be able to find the amount of magnesium in the sample. You should also be able to find the mass of the oxygen that has reacted with the magnesium. From these two masses and the molar masses of magnesium and oxygen, you can calculate the number of moles of Mg and O that are present in the final product. Then, you can calculate the formula of the magnesium oxide you made. أرجو أن ينال على إعجابكم نور حوراني
Views: 2468 Noor Hourani
We'll learn how to calculate percent composition by mass, and we'll work through a number of practice problems. To calculate percent by mass, you need to determine two things: the mass of just the element, and the molar mass of the whole compound. Then, you take the molar mass of just the element and divide it by the molar mass of the whole compound, and multiply by 100%.
Views: 704979 Tyler DeWitt
We'll learn how to calculate molecular formula for a compound when you are given its empirical formula and its molar mass. In order to do this, you need to figure out what to multiply the empirical formula by to get the molecular formula and the correct molar mass. The multiple can be determined by dividing the molar mass of the compound by the molar mass of the empirical formula.
Views: 786963 Tyler DeWitt
I created this video with the YouTube Video Editor (http://www.youtube.com/editor)
Views: 430 RMHSChem
If you're given the Percent Composition of a compound, you can find the Empirical Formula for it. I have the shortest method ever to do it, although it's not a "full solution" like your teacher probably asks for. 1. Divide each % by the atomic mass of the element 2. Divide each of THOSE answers by whatever's smallest 3. Adjust these numbers into their lowest whole-number ratio. Check me out: http://www.chemistnate.com
Views: 614926 chemistNATE
This chemistry video tutorial shows you how to determine the empirical formula from percent composition by mass in grams. This video also shows you how to determine the molecular formula from the empirical formula using the combustion analysis technique of a compound. This video contains plenty of examples and practice problems that can help you on your next upcoming worksheet assignment / quiz. Here is a list of topics: 1. Empirical Formula - Lowest Whole Number Ratio 2. Finding the empirical formula from mass in grams 3. Determining the empirical formula using percent composition by mass 4. Calculating Molecular Formula From Empirical Formula Using Molar Mass 5. Combustion Analysis - Compound with 2 elements - Carbon & Hydrogen 6. Empirical Formula From Combustion Analysis - 3 Element Compound - Carbon, Oxygen, and Hydrogen 7. Decimal Ratio Subscripts & Fractions - Converting to whole numbers
Views: 79862 The Organic Chemistry Tutor
This video demonstrates how to calculate the percent water in copper (II) sulfate pentahydrate by analysis of its chemical formula. Other Stoichiometry videos: Sandwich Stoichiometry - https://goo.gl/Cq3AKx Calculating Empirical Formulas - https://goo.gl/1GBQJB Calculating % Water of a Hydrate - https://goo.gl/hbTfYZ Empirical Formula of a Hydrocarbon - https://goo.gl/PxS2KK Formula Units of Magnesium Chloride - https://goo.gl/dMYkA8
Views: 40640 Noel Pauller
Confused about molarity? Don't be! Here, we'll do practice problems with molarity, calculating the moles and liters to find the molar concentration. We'll also have to use conversion factors to convert between grams and moles, and between milliliters and liters.
Views: 1105219 Tyler DeWitt
Abstract The purpose of this lab was to analyze precipitate with a measurement of millimeters from the test tubes that contained CuCl2 and Na3PO4 to find out the empirical formula. For this lab, we were given instructions to put a certain amount of the two reactants in the test tubes, which are CuCl2 and Na3PO4. Seven test tubes were analyzed in total that contained both Ionic reactants. We used a data table to collect and interpret our results. We compared observations with all other 6 test tubes and found out that the highest ratio was 3:2. We also observed that there was color change in the mixture of both ionic reactants, going from light blue to dark blue after adding both reactants. Therefore, by measuring the precipitate of each test tube, we found out the empirical formula.
Views: 63 Jasmine W.
There's a thing with carbon and hydrogen in it. But how many of each?! That's the kind of thing a chemist should know. So let's do some elemental analysis! Subscribe: http://bit.ly/ProfDaveSubscribe [email protected] http://patreon.com/ProfessorDaveExplains http://professordaveexplains.com http://facebook.com/ProfessorDaveExpl... http://twitter.com/DaveExplains General Chemistry Tutorials: http://bit.ly/ProfDaveGenChem Organic Chemistry Tutorials: http://bit.ly/ProfDaveOrgChem Biochemistry Tutorials: http://bit.ly/ProfDaveBiochem Classical Physics Tutorials: http://bit.ly/ProfDavePhysics1 Modern Physics Tutorials: http://bit.ly/ProfDavePhysics2 Mathematics Tutorials: http://bit.ly/ProfDaveMaths Biology Tutorials: http://bit.ly/ProfDaveBio American History Tutorials: http://bit.ly/ProfDaveAmericanHistory
Views: 34700 Professor Dave Explains
This is the first in a series of 3 lessons about the interpretation of electron impact mass spectra. This video was created for a university course in instrumental analysis in chemistry. Spectra were taken from http://webbook.nist.gov/chemistry/ and used with permission. The isotope calculator mentioned in the video can be found at http://www.sisweb.com/mstools/isotope.htm
Views: 165858 Gary Mabbott
Dimensional analysis involving moles, Avogadros number, and molarity. Reaction Stoichiometry including limiting reactants, percent yield, and percent purity. Empirical formulas and hydrate formulas from % composition or mass data. Empirical formula from combustion data.
Views: 457 Dena Leggett
This video will take you through the steps of finding the percent composition by mass of a compound. as well as determining the empirical formula from mass data. More practice to follow.
Views: 141 Andrew Baldwin
Watch to learn how to determine the empirical formula for magnetic iron oxide which is made up of 72.4% iron and 27.6% oxygen! Empirical formulas are chemical formulas that show the composition of a compound in terms of the relative numbers and types of atoms in the simplest ratio.
Views: 258 Jackie Castorino
Chemists need stoichiometry to make the scale of chemistry more understandable - Hank is here to explain why, and to teach us how to use it. Table of Contents Atomic Mass Units 2:24 Moles 5:12 Molar Mass 5:59 Equation Balancing 8:45 Molar Ratios 11:11 Crash Course elsewhere on the internet: http://www.facebook.com/YouTubeCrashCourse http://www.twitter.com/TheCrashCourse http://thecrashcourse.tumblr.com References and image licenses for this episode can be found in the Google document here: http://dft.ba/-51j2 Support CrashCourse on Subbable: http://subbable.com/crashcourse
Views: 2370904 CrashCourse
Lecture on Percent Comp. of a compounds, how to determine Empirical formulas (combustion analysis) Table of Contents: 00:00 - Percent Composition, Empirical and Molecular Formulas 00:18 - Calculating Percentage Composition 00:57 - Formulas 01:50 - Formulas (continued) 02:46 - Formulas (continued) 03:44 - Empirical Formula Determination 05:33 - Empirical Formula Determination 06:28 - Empirical Formula Determination 07:07 - Empirical Formula Determination 08:21 - Finding the Molecular Formula 08:53 - Finding the Molecular Formula 09:13 - Finding the Molecular Formula 09:54 - Determine Empirical Formulas by Combustion Analysis 12:38 - Determine Empirical Formulas by Combustion Analysis Cont. 14:12 - Determine Empirical Formulas by Combustion Analysis Cont.
Views: 828 Ethan Schnell
How to determine empirical and molecular formula IB Chemistry Past Paper Exam Qs 2016 Specimen P2 SL Q4bi ii To determine the empirical formula the most important trick is to turn the percentage compositions straight to mass by assuming you have 100g of sample. Then just calculate the number of moles using n=m/M, place these mole values into a chemical formula and then divide by the smallest number and times out to get whole numbers. The molecular formula will be a whole number multiple of this (x1, x2, or x3 etc...). Use the given molecular mass to determine what whole number multiple of the empirical formula makes the molecular formula. Calculations template can be downloaded here: http://www.mrwengibchemistry.com/ib-chemistry-exams.html PPTs and quizzes are available on: http://www.mrwengibchemistry.com/ 2016 IB Chemistry EXAM Past paper 1 SL Specimen: https://www.youtube.com/playlist?list=PLyuGdIuwJD9HyN7bwQalRK7DF_cnLcnLA 2016 IB Chemistry EXAM Past paper 1 HL Specimen: https://www.youtube.com/playlist?list=PLyuGdIuwJD9EKe4KqHNjymhVqCQfe3EU6 2016 IB Chemistry EXAM Past paper 2 SL Specimen: https://www.youtube.com/playlist?list=PLyuGdIuwJD9HFIBGI_SgolsdTe3LOdI0G 2016 IB Chemistry EXAM Past paper 2 HL Specimen: https://www.youtube.com/playlist?list=PLyuGdIuwJD9E5ken_rYSs8iqM6cU2xTSu 2016 IB Chemistry EXAM Past paper 3 SL Specimen Option A&B: https://www.youtube.com/playlist?list=PLyuGdIuwJD9H6kLiuLuGK1kLMA2aPbNJt 2016 IB Chemistry EXAM Past paper 3 HL Specimen Option A&B: https://www.youtube.com/playlist?list=PLyuGdIuwJD9F4OFCb-azbeyvJRgaTtuZW Connect with me: Facebook: https://www.facebook.com/IBChemistry2016/ Twitter: https://twitter.com/andrewweng0406 Google plus: https://plus.google.com/u/0/108611113268141564345 Pinterest: https://www.pinterest.com/mrandrewweng040/ib-chemistry/ Weibo: http://www.weibo.com/5984983999/profile?topnav=1&wvr=6&is_all=1
Views: 3149 Andrew Weng
Watch more videos on http://www.brightstorm.com/science/chemistry SUBSCRIBE FOR All OUR VIDEOS! https://www.youtube.com/subscription_center?add_user=brightstorm2 VISIT BRIGHTSTORM.com FOR TONS OF VIDEO TUTORIALS AND OTHER FEATURES! http://www.brightstorm.com/ LET'S CONNECT! Facebook ► https://www.facebook.com/brightstorm Pinterest ► https://www.pinterest.com/brightstorm/ Google+ ► https://plus.google.com/+brightstorm/ Twitter ► https://twitter.com/brightstorm_ Brightstorm website ► https://www.brightstorm.com/
Views: 597241 Brightstorm
2/25/14 lecture at COS
Views: 100 Chemistry with Mrs. K
Abstract The purpose of this lab was to be able to construct an empirical formula based on the precipitate of the substances given. Using test tubes filled with the given ratios of CuCl2 and Na3PO4 we observed the precipitate formed which is Cu3(PO4)2. After the test tubes were filled with the given ratios they were mixed and left to sit for 15 minutes to allow the precipitate to form. The precipitate formed had a larger volume when there was a greater amount of the reactant Na3PO4. The empirical formula was constructed using the largest volume of the precipitate its ratio. By:Allison Ussery Jennika Davila and Emmanuel Flores per. 1
Views: 102 Allison Nunyo
How do you name acids? We'll learn how to look at the chemical formula for an acid and then write its name. We will focus on both acids without oxygen and also acids that contain oxygen, which are sometimes called oxoacids. In order to name an acid, you need separate the H+ from the negative ion. Then you figure out the name of the negative ion, and use rules for acid compound naming. If the negative ion ends in -ide, the acid is hydro- -ic acid. If the negative ion ends in -ate, the acid is -ic acid. If the negative ion ends in -ite, the acid is -ous acid. It's also important to note that there are some exceptions: phosphoric acid, phosphorous acid, sulfuric acid and sulfurous acid.
Views: 762982 Tyler DeWitt