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Search results “Determining rate law and rate constant lab”

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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/

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Views: 559893 Brightstorm

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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

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Determination Of First Order Reaction Rate Constant For Acid Hydrolysis Of Ethyl Acetate {L
Views: 5786 KOMAL SINGH

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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

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How to calculate reaction rate from your absorbance data!
Views: 25427 kirk kawagoe

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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

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Using Excel - Graphical Method
Views: 4912 Yu Kay Law

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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

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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

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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

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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

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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

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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

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Views: 27981 ycpChemistryLabs

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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

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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

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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

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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

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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

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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

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Views: 20776 Mark Blaser

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Views: 1330 Chem Lab

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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

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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

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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

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Views: 10497 amritacreate

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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

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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

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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

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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

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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

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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

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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).

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Views: 17068 Laura McGuire

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Views: 927 Chem Lab

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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

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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

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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

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Chemical Kinetics: Rate Law Experiment

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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

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Views: 3225 Wikitechy School

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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

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Views: 795 BrimChem

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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

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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

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