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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
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: 559893 Brightstorm
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: 12832 Scott Milam
Determination Of First Order Reaction Rate Constant For Acid Hydrolysis Of Ethyl Acetate {L
 
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Determination Of First Order Reaction Rate Constant For Acid Hydrolysis Of Ethyl Acetate {L
Views: 5786 KOMAL SINGH
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: 10108 LearnChemE
Calculating Reaction Rate from Your Lab Quest Data
 
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How to calculate reaction rate from your absorbance data!
Views: 25427 kirk kawagoe
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: 5697 Nicole Langlois
Concentration-Time Data - Determination of Rate Law and Rate Constant
 
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Using Excel - Graphical Method
Views: 4912 Yu Kay Law
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: 16726 Scott Milam
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
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: 5710 UTAchemistry
Arrhenius Equation Activation Energy and Rate Constant K Explained
 
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This chemistry video tutorial focuses on the Arrhenius equation and how to derive it's many different forms within the subject of chemical kinetics. Here is a list of topics: 1. Arrhenius Equation and the Rate Constant K 2. The units of R and the activation energy 3. Rate law expression and the concentration of reactant A 4. Frequency Factor, Collision Frequency and Steric Factor 5. Rate of Reaction, Rate Constant K, and Activation Energy 6. The Effect of a Catalyst on Activation Energy and Reaction Rate 7. Slope, Ea, and R 8. Slope Intercept Form Linear Arrhenius Equation 9. Factors Affecting the rate of the reaction - concentration, temperature, catalyst, activation energy and rate constant K 10. Arrhenius Equation / Formula Graph
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
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: 46011 Michel van Biezen
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: 23412 Eric Zuckerman
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: 23463 LearnChemE
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: 287834 chemistNATE
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: 13350 Ali Hayek
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: 200428 FlinnScientific
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: 21426 chempatenaude
Advanced 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://sellfy.com/p/NbUf/ 👉 SHOP MY STEP-BY-STEP CHEMISTRY NOTES👈 https://sellfy.com/melissamaribel Thermochemistry: https://sellfy.com/p/9zWI/ Acids and Bases: https://sellfy.com/p/Ta1z/ Naming Compounds and Acids: https://sellfy.com/p/Cpof/ Dimensional Analysis, Significant Figures, and Density: https://sellfy.com/p/6AnT/ Gas Laws: https://sellfy.com/p/De81/ Stoichiometry: https://sellfy.com/p/NObu/ Redox Reactions: https://sellfy.com/p/rQsZ/ Molarity: https://sellfy.com/p/2A3h/ Limiting Reactants: https://sellfy.com/p/J2oT/ Lewis Structures: https://sellfy.com/p/HjLq/ 🧡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 know from experience that finding the right tutor isn’t always easy, so here’s 30 minutes free with Chegg tutors so you can find the right tutor. https://che.gg/melissamaribeltutors 📚 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 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
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: 138048 Ben's Chem Videos
Iodine Clock Reaction
 
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Views: 20776 Mark Blaser
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: 14530 Marazban Kotwal
Determining the Order of a Reaction
 
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How the order of a chemical reaction is determined. Also, a few examples on determining the order of a reaction with one reactant decomposing into products.
Views: 296205 Ben's Chem Videos
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: 15716 Michael Seery
Kinetics Study on the Reaction between Iodide Ions and Hydrogen Peroxide - MeitY OLabs
 
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This video channel is developed by Amrita University's CREATE http://www.amrita.edu/create ▶ For more Information @ http://amrita.olabs.co.in/?sub=73&brch=8&sim=117&cnt=1 ▶ Online Labs for School lab Experiments (Olabs) http://www.olabs.edu.in/ ▶ Learn more about Amrita University http://www.amrita.edu ▶ Subscribe @ http://www.youtube.com/amritacreate http://www.youtube.com/amritavlab ▶ Like us @ https://www.facebook.com/CREATEatAmrita Copyright © 2016 Amrita University Developed by CDAC Mumbai & Amrita University under research grant from Department of IT, Government of India Kinetics Study on the Reaction between Iodide Ions and Hydrogen Peroxide :- The speed of a reaction or the rate of a reaction is defined as the change in concentration of a reactant or product in unit time. It can be expressed as, the rate of decrease in concentration of any one of the reactants or the rate of increase in concentration of anyone of the products. The speed of a reaction or the rate of a reaction is defined as the change in concentration of a reactant or product in unit time. It can be expressed as, the rate of decrease in concentration of any one of the reactants or the rate of increase in concentration of anyone of the products. The reaction between iodide ions and hydrogen peroxide occurs in the acidic medium. In this reaction, hydrogen peroxide oxidises iodide ions to molecular iodine. If calculated amount of sodium thiosulphate is added in the presence of starch solution as an indicator to the above reaction mixture, the liberated iodine reacts with thiosulphate ions as fast as it is formed and is reduced back to iodide ions till all the thiosulphate ions are oxidised to tetrathionate ions. When thiosulphate ions are completely consumed, the liberated iodine reacts with starch solution and gives a blue colour. This video explains how to study the reaction rate of the reaction of iodide ions with hydrogen peroxide at different concentrations of iodide ions.
Views: 10497 amritacreate
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: 6283 Shawn Shields
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: 110976 SlowChem
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: 41929 chemistNATE
Experiment 20 Introduction and Sample Calculations
 
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In this video, I give an introduction to Experiment 20, which uses the method of initial rates to determine the rate law for the acid catalyzed iodination of acetone.
Views: 2027 Patrick Fleming
Chemistry - Chemical Kinetics (12 of 30) Finding the Order Using the Isolation Method
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will find the order using the isolation method.
Views: 9380 Michel van Biezen
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: 1815 Real Chemistry
Rate Law Experiment - August 2016
 
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During a chemistry lab at Oregon State University, an experiment was performed in order to determine the rate of reaction for H2O2 (hydrogen peroxide) and KI (potassium iodide).
16.2a Using a rate law
 
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Views: 927 Chem Lab
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: 6829 Farnborough Chemistry
The Equilibrium Constant
 
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065 - The Equilibrium Constant In this video Paul Andersen defines the equilibrium constant (K) and explains how it can be calculated in various reversible reactions. The equilibrium constant is a ratio of the concentration of the products to the concentration of the reactants. If the K value is less than one the reaction will move to the left and if the K value is greater than one the reaction will move to the right. Do you speak another language? Help me translate my videos: http://www.bozemanscience.com/translations/ Music Attribution Title: String Theory Artist: Herman Jolly http://sunsetvalley.bandcamp.com/track/string-theory All of the images are licensed under creative commons and public domain licensing: "File:Lightning Hits Tree.jpg." Wikipedia, the Free Encyclopedia. Accessed January 2, 2014. http://en.wikipedia.org/wiki/File:Lightning_hits_tree.jpg. "File:Nitric-Oxide-3D-vdW.png." Wikipedia, the Free Encyclopedia. Accessed January 2, 2014. http://en.wikipedia.org/wiki/File:Nitric-oxide-3D-vdW.png. "File:Phosgene Poster ww2.jpg." Wikipedia, the Free Encyclopedia. Accessed January 2, 2014. http://en.wikipedia.org/wiki/File:Phosgene_poster_ww2.jpg. "Reversible Reactions." PhET. Accessed January 2, 2014. http://phet.colorado.edu/en/simulation/reversible-reactions. "Reversible Reactions." PhET. Accessed January 2, 2014. http://phet.colorado.edu/en/simulation/reversible-reactions.
Views: 363554 Bozeman Science
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: 228 Tangerine Education
Rate Law Experiment
 
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Chemical Kinetics: Rate Law Experiment
326 - K1 Kinetics of Ester Hydrolysis
 
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0:07 Kinetics of Ester Hydrolysis 0:38 Getting bulk solutions 1:13 Preparing and running reaction 2:22 Constant temperature baths 3:06 Overall view of the experiment 3:50 Preparing for titration 5:09 Actually starting the reaction 7:50 Cleanup
Views: 26594 Chris Ambidge
determination of rate constant chemical kinetics 2 class 12 chemistry subject notes cbse
 
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determination of rate constant chemical kinetics 2 Top most best online video lectures preparations notes for class 12 chemistry CBSE IIT-JEE NEET exam +2/12thstd standard intermediate PUC college exams preparations tips and tricks all questions with solutions hydrolysis reaction catalysed hydrolysis of ester determination of rate constant of a dissociative reaction determination of rate constant of hydrolysis of ester determination of rate constant of photochemical reaction determination of rate constant of hydrolysis of ethyl acetate determination of rate constant of reaction Reaction rate and rate constant of the hydrolysis of ethyl rate constant of hydrolysis of ethyl acetate rate constant of hydrolysis of methyl acetate hydrolysis of ethyl acetate calculations Hydrolysis Definition Reaction Equation and Example What type of reaction is a hydrolysis reaction? Why is a hydrolysis reaction important? How are the macromolecules formed and how are they broken down what are the reactions? mechanism for the acid catalysed hydrolysis of esters hydrolysis reaction example hydrolysis reaction equation What is alkaline hydrolysis? Acid Hydrolysis of Esters Acid Catalyzed Hydrolysis website: http://www.wikitechy.com/ cbse ncert cisce nios ICSE wbsc WBBSE IB bse igcsen icsce aisse hslc aicte mpbse isc sslc jkbose jksbse cce hbse matric GSHSEB isc state board scert nenbse seba cgbse samacheer online school videos and lectures Higher secondary school +2 12thstd standard Andhra Pradesh (Secondary Intermediate) –inter college or junior college 2nd year Bihar (School Intermediate)-PUC 2 nd year HSE Meghalaya Mizoram Nagaland Odisha Assam Kerala Madhya Pradesh Maharashtra Manipur (Secondary Higher Secondary) Council for the Indian School Certificate Examinations the Central Board for Secondary Education the National Institute of Open Schooling Pre-primary Primary Middle/ upper-primary Senior secondary inter college Board of Secondary Education CBSE Class 12 Chemistry , CBSE class 12 , Class +2 Chemistry,AIIMS,CMC-Vellore ,CMC-Ludhiana,COMED-K,JIPMER,Manipal (MBBS),MGIMS-Wardha,AMU (MBBS),BHU Medical,BITSAT ,COMED-K,IPU-CET (B.Tech),Manipal (B. Tech),VITEEE,AMU (B. Tech),NDA Entrance with PCM (MPC),All India Engineering Entrance Exam with PCM (MPC).State Level Engineering Entrance Exams,intermediate chemistry,|neetexam,Joint Entrance Examination (JEE) Main/Advanced,,AIPMT,AIPVT,Indian Maritime University Common Entrance Test,Indian Navy B.Tech Entry Scheme.NEST / NDA / RIE CEE Integrated B Ed / GGS IP University CET / CU CET / BHU UET / HSEE / TISS BAT / Symbiosis University SET , Delhi University B El Ed Entrance CEE , UPSEE ,RIE CEE |JEE Mains / JEE Advanced / BITSAT / VITEEE / MH CET / Architecture B Arch JEE / NATA / B Arch JamiaMliaIslamia / IISER / Chennai Mathematical Institute / Statistics Entrance Exams/ NDRI Karnal / NIFTEM, NEET / AIIMS MBBS / JIPMER / AIPVT / CMC Vellore Medical Entrance test / CET Karnataka / EAMCET / Agriculture Science AIEEA - UG / Biology Entrance Exams|Punjab University entrance for B Sc Applied Biological Sciences PU CET / CET for admission at SVNIRTAR and NIOH / IPH |Hotel Management / Culinary Arts Entrance Exams NCHMCT / E CHAT / PUTHAT / Indian Culinary Institute Tirupati |Law Entrance Exams CLAT / AILET / LSAT India / Punjab University Law Entrance Test| Design Entrance Exams / NIFT / NID | Kurukshetra / UCEED / CEPT / SUPVA Rohtak / MITID DAT / Pearl Academy Admission / College of Art, Delhi University / Apeejay Institute of Design / FDDI Noida |Entrance  Chartered Accountancy Entrance Exam / CPT Management Entrance Tests IPM IIM Indore / Delhi University BMS BBE BFIA entrance JAT   ISRO Officer Recruitment Preparation |State Bank Of India SO Jobs | Staff selection Commission (SSC) |SSC Upper Division Clerk Exam |Union Public Service Commission-UPSC Online Video Lectures tamilnadu -tnpsc group 1| tnpsc group 2 tnpsc group 4 Andhra Pradesh -APPSC group 1 | APPSC group 2 | APPSC group 4 Arunachal Pradesh PSC group 1 | PSC group 2 | PSC group 4 Bihar -BSSC group 1 | BSSC group 2 |BSSC group 4 Gujarat -GPSC group 1 | GPSC group 2 | GPSC group 4 Jammu & Kashmir -JKPSC group 1 | JKPSC group 2 | JKPSC group 4 Jharkhand -JSSC group 1 | JSSC group 2 | JSSC group 4 Madhya Pradesh -MPPSC group 1 | MPPSC group 2 | MPPSC group 4 Maharashtra -MPSC group 1 | MPSC group 2 | MPSC group 4 Odisha -OPSC group 1 | OPSC group 2 | OPSC group 4 Punjab -PPSC group 1 | PPSC group 2 | PPSC group 4 Uttar Pradesh -UPPSC group 1 | UPPSC group 2 | UPPSC group 4 West Bengal -WBSSC group 1 | WBSSC group 2 | WBSSC group 4 Karnataka -KPSC group 1 | group 2 | group 4 Kerala PSC group 1 | group 2 | group 4 Rajasthan -RPSC group 1 | RPSC group 2 | RPSC group 4 public service commission exam
Views: 3225 Wikitechy School
Crystal Violet Kinetics Experiment
 
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Crystal Violet is reacted with sodium hydroxide. The change in color is tracked with a Vernier Spectrovis Plus. The absorbance is used to determine the order with respect to crystal violet. A second reaction is run with double the concentration of sodium hydroxide to show the order of hydroxide. Prior to running a Beer's Law calibration curve is constructed so that the absorbance values can be converted into concentrations. The rate order and rate constant can be found with some manipulations, some of which can be done with the Vernier Labquest 2.
Views: 2859 Scott Milam
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: 39875 Michael Seery
Kinetics: Chemistry's Demolition Derby - Crash Course Chemistry #32
 
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You can directly support Crash Course at http://www.subbable.com/crashcourse Subscribe for as little as $0 to keep up with everything we're doing. Also, if you can afford to pay a little every month, it really helps us to continue producing great content. Have you ever been to a Demolition Derby? Then you have an idea of how molecular collisions happen. In this episode, Hank talks about collisions between molecules and atoms, activation energy, writing rate laws, equilibrium expressions, reactions mechanics, and rate-determining steps. And funnel cakes are AWESOME! ***** AND NOW, A SUBBABLE MESSAGE! ***** "Jane McLauchlan, thank you for decreasing worldsuck. I love you!" - Charlotte Thornton -- Table of Contents Collisions Between Molecules and Atoms 0:00 Activation Energy 1:32 Writing Rate Laws 3:28 Rate Laws and Equilibrium Expressions 5:30 Reaction Mechanisms 8:06 Rate-Determining Steps 7:04 -- Want to find Crash Course elsewhere on the internet? Facebook - http://www.facebook.com/YouTubeCrashCourse Twitter - http://www.twitter.com/TheCrashCourse Tumblr - http://thecrashcourse.tumblr.com Support CrashCourse on Subbable: http://subbable.com/crashcourse
Views: 562725 CrashCourse
Finding units of rate constant k | Knetics | Chemistry | Khan Academy
 
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How to find the units for the rate constant k for a zero, first, or second order reaction. Watch the next lesson: https://www.khanacademy.org/science/chemistry/chem-kinetics/reaction-rates/v/experimental-determination-of-rate-laws?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-law-and-reaction-order?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
Views: 212051 Khan Academy

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