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Initial Rates Method For Determining Reaction Order, Rate Laws, & Rate Constant K, Chemical Kinetics
 
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This chemistry video tutorial provides a basic introduction into method of initial rates which is useful for determining the order with respect to the reactants and the overall reaction order. In addition, the initial rates method is useful for experimentally determining the rate law expression for a particular chemical reaction. This video explains how to calculate the value of the rate constant K and how to determine its units. This video is part of the chemical kinetics series. It contains plenty of examples and practice problems. 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 Facebook: https://www.facebook.com/MathScienceTutoring/
Experimental determination of rate laws | Knetics | Chemistry | Khan Academy
 
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Example using initial rates to find the order in each reactant, the overall order, and the rate constant k. Watch the next lesson: https://www.khanacademy.org/science/chemistry/chem-kinetics/copy-of-kinetics/v/plotting-data-for-a-first-order-reaction?utm_source=YT&utm_medium=Desc&utm_campaign=chemistry Missed the previous lesson? https://www.khanacademy.org/science/chemistry/chem-kinetics/reaction-rates/v/finding-units-of-rate-constant-k?utm_source=YT&utm_medium=Desc&utm_campaign=chemistry Chemistry on Khan Academy: Did you know that everything is made out of chemicals? Chemistry is the study of matter: its composition, properties, and reactivity. This material roughly covers a first-year high school or college course, and a good understanding of algebra is helpful. About Khan Academy: Khan Academy offers practice exercises, instructional videos, and a personalized learning dashboard that empower learners to study at their own pace in and outside of the classroom. We tackle math, science, computer programming, history, art history, economics, and more. Our math missions guide learners from kindergarten to calculus using state-of-the-art, adaptive technology that identifies strengths and learning gaps. We've also partnered with institutions like NASA, The Museum of Modern Art, The California Academy of Sciences, and MIT to offer specialized content. For free. For everyone. Forever. #YouCanLearnAnything Subscribe to Khan Academy’s Chemistry channel: https://www.youtube.com/channel/UCyEot66LrwWFEMONvrIBh3A?sub_confirmation=1 Subscribe to Khan Academy: https://www.youtube.com/subscription_center?add_user=khanacademy
Kinetics Experiment Rate Law + Activation Energy
 
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The rate law for 6I- + BrO3- + 6H+ --- 3H2O + Br- + 3I2 is determined using a clock reaction where the I2 reacts with thiosulfate until the thiosulfate runs out. Starch indicator is used to produce a blue color indicating that the iodine has reacted with all of the thiosulfate. The rate law is determined by mixing 10 mL of distilled water, 10 mL of 0.040 M KBrO3, 10 mL of 0.10 M HCl, 10 mL of 0.010 M KI and 10 mL of 0.0010 M Na2S2O3. In experiments 2-4, the amount of KI, KBrO3 and HCl are doubled and the distilled water is not added. This causes each to double in concentration for that experiment while all other concentrations remain constant. Finally the experiment is run with the same amounts as experiment #1, but at two different temperatures. This is used to measure the rate constants at these two temperatures in order to determine the activation energy for the reaction.
Views: 15106 Scott Milam
Kinetics lab - rate law determination of iodination of acetone, determining activation energy
 
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Kinetics experiment where the reaction between iodine and acetone with acid catalyst is tracked for determination of the rate law with respect to iodine, acid and acetone concentrations. The rate constant is determined and then measured at two temperatures to determine the activation energy in J/mol by plotting ln k vs. 1/T to get a slope of -Ea/R.
Views: 19537 Scott Milam
Reaction Rate Laws
 
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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: 596918 Brightstorm
Determing Rate Equation for Sodium Thiosulfate and Hydrochloric Acid
 
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Practical work to determine the rate equation for the reaction between hydrochloric acid (HCl) and sodium thiosulfate (Na2S2O3). The disappearing cross experiment. No commentary.
Views: 8570 Farnborough Chemistry
Reaction Rates! Determination of Rate Law with Sodium Thiosulfate and Hydrochloric Acid
 
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This video highlights methods in which the rate law and reaction orders for a chemical reaction can be determined using colorimetry. This is a collaborative project between Nicole Langlois, Nadine Hudson, and Stephanie Virgulto - students enrolled in the Spring 2015 CHEM 1117 Honors Lab course at the University of New Haven. Screen captures were made possible through the Screencast-O-Matic program. The background music was taken from the Marvel Cinematic Theme Song Universe at https://www.youtube.com/watch?v=Dnik1H_8cbg, all rights reserved to their respective owners.
Views: 6307 Nicole Langlois
Kinetics:  The Rate Law from Graphing Data
 
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Sample concentration vs. time data is analyzed to determine the reaction order, rate law and rate constant.
Views: 27607 Eric Zuckerman
Chemistry Rate Law Example Problem
 
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Erika Tan walks through a past AP Chemistry free response problem regarding chemical kinetics. TRANSCRIPT: This question actually has a couple parts to it. So first of all, it’s asking us to find the order with respect to reactant A, find the order with respect to reactant B, find the rate law, calculate the rate constant, and calculate the initial rate of experiment #4 which is the question mark. I just copied this chart from the question that I took it from, so let’s start on the first part: find the order of the reaction with respect to A. So here I’m going to look down this column, which gives me the initial concentration of A, and the units are molarity (which is moles/liter), and then, I’m going to see, since I’m trying to find the order with respect to A, I’ll have to find two experiments that have about the same concentration of B. So I’m looking at experiments 2 and 3 right now because .137 and .136 are basically the same thing. Since I’m keeping B constant, I’ll be able to see what happened to A to change the rate. But by how much? So I’m just going to do .136 divided by .034, that’s what I’m getting here, and I see that this, experiment #3, is just the concentration of A times 4. So let’s not forget that. This is times 4. Since we know that this is being constant, and we know that this is being multiplied by 4, let’s see what happens to the rate. So I see 1.08 times 10^-2 and 1.07 times 10^-2. Well, those are basically the same thing, I just see the 8 and the 7 which only has a difference of 1. So, we know the concentration of A has no effect on the rate, since rate stays constant. So that means the order of reactant A is 0, since changing the concentration of A does not change the rate. Now let’s look at B. We have to find 2 experiments where A is being held constant. I see experiments 1 and 2 because this change in concentration is almost nothing. Let’s see what happens when we do .137 divided by .034. That gives us 4 again, so we’re multiplying .034 by 4 to get .137. And let’s see what happens to the rate. Again, these two don’t look the same so I’m going to divide and see what happened to it. .108 times 10^-2 divided by 6.67 times 10^-4. And that gives us about 16. So this times 16 gives you that. Obviously, there’s been a change in rate, so what is the order of B? Well, this concentration of B has been multiplied by 4. The rate has been multiplied by 16. To find the order, we’ll have to do 4 to what exponent gives you 16? X has to be 2, because 4 squared gives you 16. That means 2 is the order of B. So now we have A is 0 order, and B is second order. Let’s write the rate law. It’s just rate=k (which is a constant) and we’ll have concentration of A to the 0, which anything to the 0th power is just 1, so you don’t even have to write that, and then we have concentration of B squared. That’s because the order of B is 2, and we have to write it as an exponent. Now it’s asking us to calculate the rate constant next. All we have to do is take the rate law that we just wrote, plug in some numbers that you can just pick from the table, and calculate k, which is the rate constant. So, I’m just going to choose experiment #1 because it’s the first one on the chart. So we have our rate law, rate=k[B]^2, and if you plug in what you have for experiment 1, we see that the rate is this, 6.67 times 10^-4 = k times [B] which is .034, and don’t forget we have to square it from the rate law. We have our answer for k. And all we have to do is calculate the initial rate for experiment number 4 which it doesn’t give you on the table so let’s use the rate law and rate constant that we just got. So rate = .577 because that’s what we got for k, times concentration of B squared. So we see that for experiment #4, the concentration of B is .233, so all we have to do is rate = .577 times .233 squared. Easy. Now let’s plug it into our calculator and that gives us about 3.13 times 10^-2.
Views: 548 Tangerine Education
Iodide Persulfate Kinetics
 
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Pre-practical lab for iodide persulfate experiment to determine the rate constant, using the titration by thiosulfate method.
Views: 18541 Michael Seery
DON'T MISS THIS Rate Law and Rate Constant Question
 
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If you are given a table where all the trials are completely different and don’t follow a pattern, don’t worry I’ll show you how to determine the rate law and rate constant. You will also learn how to figure out the rate constant units with ease! 📗 FREE CHEMISTRY SURVIVAL GUIDE https://melissa.help/freechemguide 🙋‍♀️🙋‍♂️GOT A QUESTION? ASK ME HERE https://melissa.help/me 👉 SHOP MY STEP-BY-STEP CHEMISTRY NOTES👈 https://melissamaribel.com/ -Thermochemistry Notes https://melissa.help/thermonotes -Acids and Bases Notes https://melissa.help/acidbase1notes -Naming Compounds and Acids Notes https://melissa.help/namingnotes -Dimensional Analysis, Significant Figures, and Density Notes https://melissa.help/sigfignotes -Gas Laws Notes https://melissa.help/gaslawsnotes -Stoichiometry Notes https://melissa.help/stoichnotes -Redox Reactions Notes https://melissa.help/redoxnotes -Molarity Notes https://melissa.help/molaritynotes -Limiting Reactants Notes https://melissa.help/limreactnotes -Lewis Structures Notes https://melissa.help/lewisnotes -Kinetics Notes https://melissa.help/kineticsnotes 🧡SHOW YOUR SUPPORT ON PATREON https://www.patreon.com/melissamaribel 👍MELISSA'S FAVORITES ON AMAZON https://www.amazon.com/shop/chemistrywithmelissamaribel --OTHER RESOURCES TO HELP YOU GET THROUGH SCHOOL-- 🙌 This was my go-to homework help when I was in school. Chegg Study is one of my favorites. https://che.gg/melissamaribelstudy 📚 I made the mistake of buying all of my textbooks, I wish I had the option of renting them. Thankfully you do, with Chegg Textbook Rentals. https://che.gg/melissamaribelrentals 💰 If you bought a textbook and don’t want the hassle of selling it, Chegg can do the work for you, with Chegg Buyback. https://che.gg/melissamaribelbuyback 📝 QUICKSTUDY REFERENCE GUIDES ⬇️ 📕 CHEMISTRY BREAKDOWN AND REVIEW https://amzn.to/2t50xWx 📙 CHEMISTRY EQUATIONS AND ANSWERS https://amzn.to/2MPjC88 📘 CHEMISTRY TERMINOLOGY https://amzn.to/2t9cv1o DISCLAIMER: Some links in the description are affiliate links, which means that if you buy from those links, I’ll receive a small commission. This helps support the channel and allows me to continue making videos like this. Thanks for the support! 💁‍♀️ HI I'M MELISSA MARIBEL I help students pass Chemistry. I used to struggle with this subject, so when I finally graduated with a bachelor's degree in Chemistry, I became a tutor so that you wouldn't have to struggle like I did. I know that with the right help, YOU CAN LEARN ANYTHING! 👋 FOLLOW ME Instagram: https://www.instagram.com/hellomelissam/ Facebook: https://www.facebook.com/hellomelissam/ Twitter: https://twitter.com/hellomelissam
Views: 2694 Melissa Maribel
Finding the Rate Law using Method of Initial Rates Experiments + Example (Part 3)
 
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Dr. Shields further discusses the differential rate law and the initial instantaneous rate. How to determine the rate law for a reaction using the method of initial rates is discusses with an example. General Chemistry
Views: 7041 Shawn Shields
Chemistry - Chemical Kinetics (15 of 30) Finding Rate Law & Rate Constant, k
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will determine the rate law and the rate constant, k.
Views: 48501 Michel van Biezen
How to Find the Rate Constant of a Reaction (Given Table)
 
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How do you find the rate constant of a reaction, if all you're given is a table of kinetic data (concentrations and times)
Views: 310286 chemistNATE
Kinetics: Rates, Rate Law, Rate constant, k
 
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Average rate, determining ANY Rate Law from experimental data
Views: 16396 Michele Berkey
Calculating the Reaction Rate using the Rate Law- Example (Pt 3of 3)
 
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Dr. Shields demonstrates how to calculate the rate of reaction for new concentrations of reactants using the rate constant (with units) and orders of each reactant derived from initial rates experimental data (done in parts 1 and 2). Part 3 of 3. General Chemistry
Views: 2173 Shawn Shields
Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid
 
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Vary the concentrations of reactants and measure the time it takes for product to appear. This video is part of the Flinn Scientific Best Practices for Teaching Chemistry Video Series, a collection of over 125 hours of free professional development training for chemistry teachers - http://elearning.flinnsci.com ATTENTION: This demonstration is intended for and should only be performed by certified science instructors in a safe laboratory/classroom setting. Be sure to subscribe and check out more videos! Subscribe: https://www.youtube.com/channel/FlinnScientific/ Facebook: https://www.facebook.com/FlinnScientific/ Website: https://www.flinnsci.com/
Views: 230904 FlinnScientific
Chemical Kinetics Rate Laws – Chemistry Review – Order of Reaction & Equations
 
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This general chemistry study guide video lecture tutorial provides an overview of chemical kinetics. It contains plenty of examples, practice problems, and conceptual questions to help you to master the course. This video is especially helpful to those taking AP chemistry in high school or general chemistry in college. Here is a list of topics: 1. How to calculate the rate of the reaction using the change in concentration and time 2. Determining the order of a reactant and the overall order of the reaction using the method of initial rates. 3. How to determine the rate equation or rate law expression 4. Calculating the rate constant K and the units of K 5. Understanding the difference between the first order, second order, and zero order reaction. 6. Equations and formulas for zero order, first, and second order reactions 7. Half Life Formula, Initial Concentration of A and Rate constant K 8. Factors affecting reaction rate – concentration, temperature, and catalyst 9. Relationship between the rate of the reaction and the concentration 10. Rate constant K, temperature, catalyst, activation energy and potential energy diagrams 11. Forward activation energy vs reverse activation energy 12. Arrhenius Equation 13. Half Life Problems and Half Life Method 14. Collision frequency, steric factor, and frequency factor 15. Reaction Mechanism – Slow Step – Rate Determining Step 16. How To Find the Intermediate and Catalyst in a Reaction Mechanism
Reaction Order & Rate Constant (#15.11)
 
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Determine the order of reaction with respect to its reactants, find the rate constant, and calculate the rate at given concentrations. Based on experimental data. Kotz, et al. 7th ed. #15.11
Views: 116871 SlowChem
Differential Analysis: Determining a Rate Law
 
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Determine the rate law for a reaction occurring in a batch reactor using differential analysis. Made by faculty at the University of Colorado Boulder, Department of Chemical and Biological Engineering. Check out our Kinetics/Reactor Design playlists: https://www.youtube.com/user/LearnChemE/playlists?view=50&flow=list&shelf_id=7 Are you using a textbook? Check out our website for videos organized by textbook chapters: http://www.learncheme.com/screencasts/kinetics-reactor-design
Views: 11526 LearnChemE
Concentration-Time Data - Determination of Rate Law and Rate Constant
 
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Using Excel - Graphical Method
Views: 5181 Yu Kay Law
Determination of rate constant of a second order reaction with equal initial concentrations
 
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This video describes an experimental (laboratory) method in chemistry (Chemical Kinetics) to determine rate constant of the reaction between potassium persulphate and potassium iodide using their solutions with equal initial concentrations at room temperature. The reaction is a second order reaction.
Views: 17777 Marazban Kotwal
Reaction Rate Law (Example)
 
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Determines the reaction rate law from initial rate data for a liquid-phase reaction. Made by faculty at the University of Colorado Boulder, Department of Chemical & Biological Engineering. Check out our Chemistry playlist: https://www.youtube.com/playlist?list=PL4xAk5aclnUi1CEFNwjcheMgyWe8BwuLS Check out our website for screencasts organized by popular textbooks: http://www.learncheme.com/screencasts/chemistry
Views: 26947 LearnChemE
Crystal Violet Lab
 
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Theory and analysis for the Kinetics of Fading Dye experiment in AP Chemistry ... with the system flooded for one reactant.
Views: 24050 chempatenaude
AP Chemistry Investigation #11: Rate Law of the Fading of Crystal Violet.
 
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This video is about the AP Chemistry Investigation #11: What is the Rate Law of the Fading of Crystal Violet Using Beer's Law? In this video you will learn how to determine the pseudo-rate order in concentration of Crystal Violet in the presence of sodium hydroxide using Beer-Lambert Law. The reaction between the CV and sodium hydroxide results in a colourless species which will lead to fading the colour of the original solution. Monitoring the absorbance of CV, we will be able to monitor the change on its concentration during the course of the reaction. Students studying Chemistry at different levels could highly benefit from this video.
Views: 15463 Ali Hayek
Finding rate constants and order with excel 2013 - Real Chemistry
 
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In this video you will learn how to plot the concentration of reactants vs time to determine the rate order and rate constant of a chemical reaction. This is accomplished by using integrated rate laws. For example, if a plot of concentration vs time is linear, then the reaction is a zeroth order reaction and the slope of the best fit line is the rate constant (times negative 1). If a plot of the natural log of concentration vs time is linear, then the reaction is first order and the slope is once again the rate constant (times negative 1). Lastly, if the plot of one over concentration vs time is linear, then the reaction is second order and the rate constant is the slope (not negative in this case).
Views: 2834 Real Chemistry
Kinetics 1: Finding the Order, Rate Equation & Rate Constant
 
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Here I look at 3 examples of how the rate equation can be obtained from experimental runs. The order of the reaction for each of the reactants is determined, allowing the rate equation to be constructed. In the third example I rearrange the rate equation to make the rate constant (k) the subject of the equation. I then work out its value and units. In the next video "Kinetics 2" I look at 3 further examples, which are a little more difficult.
Views: 2342 FranklyChemistry
Rate Law for a Mechanism with a Fast Initial Step
 
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How to determine the rate law for a mechanism with a fast initial step. Remember, the overall rate law must be determined by experiment. Therefore, the rate law must contain no reaction intermediates.
Views: 151997 Ben's Chem Videos
Chemical Kinetics | Pseudo Rate Order.
 
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This video is about Chemical Kinetics and explains in details the Reaction Rate Laws. Students studying Chemistry at different levels could highly benefit from this video. This video is the fourth of a complete series that explains different topics on chemical kinetics that include: 1- Chemical Kinetics: Reaction Rates & Rate Law. https://www.youtube.com/watch?v=r6Pdjc_xVvM 2- Chemical Kinetics: Determining the Form of the Rate Law. https://www.youtube.com/watch?v=bHX80yjsHus 3- Chemical Kinetics: Integrated Rate Law. https://www.youtube.com/watch?v=orV6LI3EEhg 4- Chemical Kinetics: Pseudo Rate Law. https://www.youtube.com/watch?v=2VLA3xoPSAI 5- Chemical Kinetics: Reaction Mechanism. https://www.youtube.com/watch?v=emEWPOamI7g 6- Chemical Kinetics: A Model for Chemical Kinetics & Catalysis. https://www.youtube.com/watch?v=952gAYVygZs
Views: 11109 Ali Hayek
Iodine Clock Reaction
 
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Views: 28361 Mark Blaser
Kinetics Part 1: Iodine Clock Reaction
 
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Discussion and data for kinetics part 1.
Views: 43468 Shaun Shelton
How2: Determine orders, rate equation and rate constant using the initial rates method
 
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The initial rates method shows the effect of varying reactant concentrations on the initial rate of reaction. Using this data we can determine the order with respect to each reactant, and hence the rate equation. We can then use the experimental data to calculate the value of the rate constant.
Views: 18181 Andrew Crookell
Iodination of Acetone (2011aR)
 
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Description of the first week of the Rate and Activation Energy of the Iodination of Acetone experiment. {re-edited to fix audio/video sync problems.} Some of the technical aspects of the experiment are discussed on my blog (http://msumgenchem.blogspot.com/2012/02/kinetics-experiments-nuts-and-bolts.html)
Views: 9455 drbodwin
Calculate Activation Energy (Slope OR formula)
 
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Given two rate constants at two temperatures, you can calculate the activation energy of the reaction. In the first 4m30s, I use the slope formula (y2-y1 / x2-x1) In the last half, I use the Arrhenius equation to solve for Ea directly.
Views: 55374 chemistNATE
Performing the Iodine Clock Reaction
 
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This experiment demonstrates the iodine clock reaction between iodide and persulfate ions, using thiosulfate as the 'clock'. After some introduction details, three experiments are performed: studying the effect of concentration to determine the orders of reactants (3:01), studying the effect of temperature to determine the activation energy (7:47) and studying the effect of solvent polarity (9:42).
Views: 42776 Michael Seery
Rate law and reaction order | Knetics | Chemistry | Khan Academy
 
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Using method of initial rates to determine the order of a reaction. Watch the next lesson: https://www.khanacademy.org/science/chemistry/chem-kinetics/reaction-rates/v/finding-units-of-rate-constant-k?utm_source=YT&utm_medium=Desc&utm_campaign=chemistry Missed the previous lesson? https://www.khanacademy.org/science/chemistry/chem-kinetics/reaction-rates/v/rate-of-reaction?utm_source=YT&utm_medium=Desc&utm_campaign=chemistry Chemistry on Khan Academy: Did you know that everything is made out of chemicals? Chemistry is the study of matter: its composition, properties, and reactivity. This material roughly covers a first-year high school or college course, and a good understanding of algebra is helpful. About Khan Academy: Khan Academy offers practice exercises, instructional videos, and a personalized learning dashboard that empower learners to study at their own pace in and outside of the classroom. We tackle math, science, computer programming, history, art history, economics, and more. Our math missions guide learners from kindergarten to calculus using state-of-the-art, adaptive technology that identifies strengths and learning gaps. We've also partnered with institutions like NASA, The Museum of Modern Art, The California Academy of Sciences, and MIT to offer specialized content. For free. For everyone. Forever. #YouCanLearnAnything Subscribe to Khan Academy’s Chemistry channel: https://www.youtube.com/channel/UCyEot66LrwWFEMONvrIBh3A?sub_confirmation=1 Subscribe to Khan Academy: https://www.youtube.com/subscription_center?add_user=khanacademy
Pseudo First Order Reactions - Kinetics
 
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In this video we want to discuss the concept of Pseudo first order reaction in Kinetics. Let's take a look at an example: Given a reaction is first order with respect to both reactants A and B. For an experiment, where [A] = 0.01 moldm-3 and [B] = 0.50 moldm-3, the half life was determined to be 10 minutes. What is the new half life when the concentration of B is changed to 1.00 moldm-3? 1. Determine rate equation Let's first write down the rate equation based on the order of the reaction with respect to A and B. Since order is 1 with respect to both reactants then the rate equation is given as: rate = k [A][B] The overall order of the reaction is 2, which makes it difficult for us to determine half life as we know that half life is not constant for overall order 2 reaction. In fact, in A Level Chemistry syllabus we are only required to find half life for first order reactions. This means that the question is hinting to us that in order for us to determine half life for a second order reaction, we need to change this reaction into a first order reaction. That's where the concept of pseudo first order reaction comes in. 2. Criteria for Pseudo First Order Reaction Once we suspect the question is about pseudo first order reaction we can verify this by looking out for one of these criteria: a. excess reactant - the concentration of excess reactant is treated as constant since the change in the amount of excess reactant is negligible as the reaction proceeds. b. catalyst - the concentration of catalyst is constant as it is chemically unchanged at the end of the reaction. For this question we notice that the concentration of B is 50 times more than concentration of A. So we can treat the concentration of B as constant and make it part of rate constant k. So what we have effectively done is to change an overall order 2 reaction and make it appear like an order 1 reaction. Hence the name pseudo first order reaction. 3. Determine Half Life Since now the reaction is first order, half life is a constant and we can write it in terms of the original rate constant k and concentration of B. From the expression we know that half life is inversely proportionate to concentration of B. Comparing the 2 experiments, when we double the concentration of B from 0.5 moldm-3 to 1.0 moldm-3, we will expect the half life to be halved from 10 minutes to 5 minutes. For the detailed step-by-step discussion on how to apply Pseudo first order reaction concept, check out this video! Topic: Kinetics, Physical Chemistry, A Level Chemistry, Singapore Found this video useful? Please LIKE this video and SHARE it with your friends! SUBSCRIBE to my YouTube Channel for new A Level Chemistry video lessons every week at https://www.youtube.com/ChemistryGuru Any feedback, comments or questions to clarify? Suggestions for new video lessons? Drop them in the COMMENTS Section, I would love to hear from you! Find out more about my JC2 and IP Year 6 Chemistry Classes at Bishan @ https://chemistryguru.com.sg/jc2-class -~-~~-~~~-~~-~- Please watch my latest video: "Valence Shell Electron Pair Repulsion (VSEPR) Theory and Shapes of Molecules" https://www.youtube.com/watch?v=q_NeyW5pe-Y -~-~~-~~~-~~-~-
UTA-442: Chemical Kinetics: Determining the Rate Law for a Chemical Reaction (Chem1442)
 
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This UTA Chem experiment determines the rate law for a chemical reaction between brilliant blue dye and bleach.
Views: 6120 UTAchemistry
Writing Rate Laws - Explained
 
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This video is about Writing Rate Laws - Original
Views: 1073 Chem Academy
16.2a Using a rate law
 
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Views: 2404 Chem Lab
Methods to determine order of reaction, integrated rate law ( zero order) || #Kinetics|| In Hindi
 
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Here I have broadly discussed the methods to determine order of reaction experimentally. basically there are two methods and these are as following 1. #method_of_initial_rate 2. #method_of_isolation secondly I have given a broad explanation on why we integrate the rate laws and what are the integrated rate expressions for various order reaction. after 1 or 2 lessons I will upload a video only for problems. so stay tuned for that. If you have not seen my previous videos then go through the links video 1 basic intro to chemical kinetics: https://youtu.be/-Km4bAm9dqQ video 2:rate laws, order of reaction and molecularity of reaction: https://youtu.be/3zLpmg7nU7s if you want to connect with me in social media then click the links facebook: https://www.facebook.com/debashis.panda.144 instagram: https://www.instagram.com/debashis.panda/?hl=en twitter: https://twitter.com/debashispanda13 keep supporting me, that will motivate me to make these videos for you guys. thank you
Views: 1264 Chem Infusion
How to determine the rate law from a table of trials - Real Chemistry
 
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In this video you will use the method of initial rates to determine the rate law for the decomposition of ozone. The method of initial rates involves using a series of experiments (trials) where you measure the concentrations of different chemical species and measure the rate of the reaction. If these trials are done multiple times you can use the data to determine the rate law. For example, if trial 2 doubles the concentration of reactant A compared to trial 1 and this doubles the reaction rate, we can say that the reaction is 1st order with respect to reactant A. If trial 3 doubles the concentration of just reactant B and this quadruples the rate, we can say that the reaction is 2nd order with respect to reactant B.
Views: 1383 Real Chemistry
Kinetics:  Activation Energy Determination from Experiment
 
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The activation energy of a reaction is determined by graphical means using experimental data.
Views: 14852 Eric Zuckerman
AP chemistry kinetics lab green food coloring/bleach
 
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Green food coloring is oxidized with sodium hypochlorite. The absorbance vs. time is shown live using a vernier spectrovis plus spectrophotometer. Data is plotted in excel separately to confirm that the reaction is 1st order and rate constant is obtained.
Views: 3791 Scott Milam