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Iodine Clock Reaction
 
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Views: 20844 Mark Blaser
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: 39926 Michael Seery
Kinetics Part 1: Iodine Clock Reaction
 
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Discussion and data for kinetics part 1.
Views: 37276 Shaun Shelton
Iodine Clock - Measuring the rate of a reaction by initial rate
 
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I want to help you achieve the grades you (and I) know you are capable of; these grades are the stepping stone to your future. Even if you don't want to study science or maths further, the grades you get now will open doors in the future. Get exam ready for GCSE Maths https://www.primrosekitten.com/pages/get-exam-ready-gcse-maths Get exam ready for GCSE science AQA https://www.primrosekitten.com/pages/get-exam-ready-gcse-science-aqa Edexcel https://www.primrosekitten.com/pages/get-exam-ready-gcse-science-edexcel To help you get even better grades I’ve written a lot of e-books, packed full of loads of excellent questions to help you study. Because the best thing you can do is practice. Visit my website for e-books, flashcards and extension questions https://www.primrosekitten.com Combined Science required practical book http://geni.us/DOshu Biology required practical book http://geni.us/2aGmjIL Chemistry required practical book http://geni.us/lepsNQ Physics required practical book http://geni.us/oeQPxAO Revision Guide for AQA Printed by Amazon http://geni.us/tEE3 Extended Revision Guide for AQA Printed by Amazon http://geni.us/j2VJY Revision Guide for Edexcel Printed by Amazon http://geni.us/qBugS Extended Revision Guide for Edexcel Printed by Amazon http://geni.us/uDhSd iGCSE Revision Guide for Edexcel Printed by Amazon http://geni.us/xM0QDz iGCSE Extended Revision Guide for Edexcel Printed by Amazon http://geni.us/ze3XKo3 What I’m Reading https://www.primrosekitten.com/collections/what-im-reading Suggested science reading that isn't subject specific https://www.primrosekitten.com/collections/awesome-science-reading Physics Reading List... https://www.primrosekitten.com/collections/reading-for-a-level-physics Biology Reading List... https://www.primrosekitten.com/collections/reading-for-a-level-biology Chemistry Reading list... https://www.primrosekitten.com/collections/reading-for-a-level-chemistry Some of the links in here are affiliate links, where is get a small percentage of any money spent, if you like my channel and want to support my work, clicking these is an easy way to do it. The 'whole of the topic in … minutes' videos DO NOT comprehensively cover everything you need to know for your exams. It would be impossible to include 2 years of teaching in 1 hour. These should NOT be your only source of revision https://youtu.be/K6d4oOq-pmU My exam predictions are just GUESSES!! I don't have any insider knowledge just years of looking at exam papers. Disclaimer; You should not carry out any of these practical’s without carrying out a full risk assessment of your own first. I am human, and I make mistakes, please point out any that you find and there is no need to follow that with a load of abuse. TuitionKit allows you to schedule your revision videos, mine and loads of other great YouTubers! http://bit.ly/2yYIxxG PhET Interactive Simulations University of Colorado Boulder https://phet.colorado.edu Music; Something Elated by Broke For Free. From the Free Music Archive, CC BY Images from; Classroom Core (TpT), Hidesy Clipart (TpT), The Cher Room (TpT), The Triple Point (TpT), Ninja Woman (TpT), The Painted Crew (TpT) Teacher's Clipart (TpT) Shutterstock
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: 12852 Scott Milam
Initial rates and the iodine clock
 
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Tick tock goes the Iodine clock! Well not quite. Explore this video to find out how we can measure the initial rate from reactions and how we can use clock reactions to do the same too. Find out how we can use this to find out the order of the reaction.
Views: 20972 Allery Chemistry
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: 16767 Scott Milam
#UTeachARScholarship - Multi Step Iodine Clock Reaction
 
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Today, I demonstrate the Multi-Step Iodine Clock Reaction. With Meta-Sulfate and Iodate w/ starch mixed together, there are reactions taking place as the liquid is blank. The final reaction is noticed by when the liquid changes into a different color. #UTeachARScholarship
Chemistry experiment 28 - Iodine clock reaction
 
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Famous iodine clock reaction: oxidation of potassium iodide by hydrogen peroxide. Mixture A: - 10 mL 2.0 M sulphuric acid - 10 mL 3% hydrogen peroxide - 80 mL water Mixture B: - Solution of 0.04 g sodium thiosulfate pentahydrate in 20 mL water - Solution of 0.9 g potassium iodide in 5 mL water - 4 mL starch solution - 71 mL water
Views: 205222 koen2all
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
Rate Law Lab part 2 of
 
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Problem Statement: How much iodine is produced by reaction (3) while reaction (6) is still occurring? Express this result in terms of concentration of iodine. Hints: Reaction (6) stops when the thiosulfate is consumed. Reaction (6) converts the iodine to iodide which is CLEAR. Reaction (3) produces iodine which should turn the solution BLUE. So you won't see blue until the thiosulfate is consumed. The stoichiometry of reaction (6) will indicate how many moles of iodine were supplied by reaction (3) during the time interval when the solution was CLEAR and the stopwatch was running. So your job is to find out how much iodine was produced by reaction (3) during this time interval. This should then be converted to a molar concentration (mol/L) because that is the convention The next video will discuss how to calculate the reaction rates and then you'll have 5 rates (one for each trial). These calculations will be used to determine 'p' and 'q'.
Views: 166 Benjamin Catlin
Iodine Clock Reaction Chemical Experiment!
 
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Hello everyone. Today we will have a very unusual chemical reaction, called "Egyptian night" or the simplified version of the chemical pendulum. First, let's take a beaker and pour there a small amount of potassium iodide and sodium thiosulfate. Next dissolve this mixture into a 100 ml of water. Take a second beaker and dissolve there a little soluble potato starch. First, dissolve starch in a cold water, then pour boiling water into the beaker, to better dissolve starch. The solution becomes slightly cloudy. Next, pour starch solution to the first solution, where we have a mixture of potassium iodide and sodium thiosulfate. We get a little cloudy solution. Next, let's make a second working solution. That solution may be of a various concentrations. For this purpose I poured into each beaker a different amounts of 30% hydrogen peroxide, solution was acidified and the acid solution was diluted to 40 ml. We now carry out the reaction. I set the clock so you can see how the reaction occurs. In the main beaker I poured 20ml of the first working solution, and now I'm pouring the second working solution into the beaker. Time passes and the solution rapidly becomes black. The color change is a reaction between iodine and starch, starch as an indicator of iodine. Now take two beakers of the first working solution. Now, however, the second solution is with different concentrations and the reaction time can change. One, two, three, and mix solutions. The first solution reacts rapidly, but the second one is a bit longer. This reaction is quite beautiful and spectacular. You can play long enough with it. And now let's look at the color change in a slow motion. Facebook: https://www.facebook.com/thoisoi2 Patreon: https://www.patreon.com/Thoisoi?ty=h Music: http://audiomicro.com
Iodine clock reaction year 13 A-Level Chemistry
 
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An explanation of one of the iodine clock reactions. Part of the rates topic in A-Level Chemistry.
Views: 8484 Mr C Dunkley
Rate determining step
 
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Rate determining step can seem difficult to work out. But with this simple explanation you should have no more problems with this exam favourite. Come complete with a cake method too. Take a look to see what I mean!
Views: 26714 Allery Chemistry
Study of an Iodine Clock Reaction - WJEC A Level Experiment
 
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Studying the kinetics of the oxidation of iodine ions by hydrogen peroxide in acid solution. Filmed at Olchfa School. Music: Straight by Bensound
Views: 3780 SpaceyScience
clock reaction kinetic demo
 
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clock reaction kinetic demo
Views: Randy Mcclay
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: 200948 FlinnScientific
Clock Reactions | A-level Chemistry | OCR, AQA, Edexcel
 
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https://goo.gl/HesNiM to unlock the full series of AS, A2 & A-level Chemistry videos created by A* students for the new OCR, AQA and Edexcel specification. This video will focus on: What are Clock Reactions, The Iodine Clock Reaction, How do we measure rate from clock reactions, Summary.
Views: 1535 SnapRevise
Kinetics Clock Rxn Lab-3 Trials
 
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Sample data for chemistry students to use for determining the rate order of [H2O2] in the iodine clock reaction. Created on March 9, 2012
Views: 173 eknispel
Clock Reaction Part 2
 
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Describes the three parts in the Clock Reaction Lab
Views: 2893 Sehat Nauli
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: 5707 Nicole Langlois
2 CHM590Demo 2014 06 16 Iodine Clock
 
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2. Iodine Clock Iodine (I2) when added to starch produces a dark blue complex. Classic test for starch, Here we control the formation of iodine by varying the starting amount of potassium iodate (KIO3). Reaction i. Iodate and bisulfite reaction slowly produces iodide ion: This is the rate determining step. IO3- + 3 HSO3-  I- + 3 HSO4- ii. iodate in excess will oxidize the iodide generated above to form iodine, IO3- + 5 I- + 6 H+  3 I2 + 3 H2O iii. bisulfite reduces immediately back to iodide I2 + HSO3- + H2O  2 I- + HSO4- + 2 H+ When Bisulfite is consumed iodine will survive to form dark blue complex with starch.
Views: 120 Arb Anu
Lab Experiment #19: Effect of Concentration on the Reaction Rate.
 
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This video is about the AP Chemistry Laboratory – Experiment #19: Effect of Concentration on the Rate of a Chemical Reaction. In this video you will learn how to determine the initial rate of a reaction by monitoring the amount of a product produced. In this case will be the hydrogen produced from the reaction between magnesium and hydrochloric acid. Moreover, you will be able to study the effect of concentration on the reaction rate.
Views: 12224 Ali Hayek
PAG10
 
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Video looks at the planning of an experiment and the subsequent analysis of results to show that a reaction is first order with respect to a particular reactant.
Views: 3995 MaChemGuy
Chemical Kinetics
 
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A video demonstrating the CHEM 1001 experiment on chemical kinetics
Views: 36204 Bob Burk
Reaction Kinetics in Blue
 
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Explore the effect of temperature and concentration on the rate of fading of methylene blue. 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: 29741 FlinnScientific
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: 15785 Michael Seery
Iodine Clock Analysis
 
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This video describes how to analyze and graph the data for our Iodine Clock Reaction experiment in Grade 12 chemistry.
Views: 4011 chempatenaude
BCLN - Iodine Clock Reaction - Chemistry
 
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Chemistry 12 - Iodine Clock Reaction Lab http://www.BCLearningNetwork.com. 0:03ok today we're going to be doing the 0:06iodine clock reaction this is actually a 0:10really awesome ranch the first time I 0:12saw this one it was 0:14Wow remember the first like we did in 0:17the first unit rates of reaction we 0:21found out that temperature concentration 0:25and surface area affects the reaction 0:28what we're going to be doing today is 0:30we're going to be doing and using 0:32different reactions to cover the same 0:34topics but in this case the reaction 0:38takes place in two steps in the first 0:41step we notice the ID ati on reacts with 0:45the buy/sell flight to create the I 0:48minus ion in the second reaction the 0:52idea I'm reacts with the i- produced to 0:56produce a wonderful blue color now the 0:59neat thing about this is if we vary the 1:01concentrations we can change the rate of 1:05the reaction what we'll be doing is 1:07measuring the different rates of 1:08reaction at different concentrations so 1:12let's see what happens we'll just zoom 1:13in here so mixing solution a task my day 1:21with solution be 1:29remember to watch please 1:35Wow is not amazing i tell you the first 1:38time i saw that i was impressed 1:41we're just going to stay soon and we'll 1:45do the other parts of the lab the second 1:49test we're using is now nine mils gaseum 1:54I'd a dilated to 10 mils also mixing it 1:58with 10 mils of solution be remember to 2:05mix thoroughly I tell you every time I 2:11see it I'm still impressed or moving 2:14aside what we can you could we can use 2:17them the clock on the player on the 2:21native player that you're using to 2:23measure the rate what I'll also be doing 2:25does not make sure to put up a table for 2:30you with the times 2:36you'll notice one thing right away is 2:40that the reactions are taking a little 2:44bit more time to the good mix and wait 2:53for it and notice the appearing of this 2:57time the blue color takes a little bit 3:00longer now it's up to you to think about 3:06why 3:07and lastly we're down to three mils of 3:12potassium iodate done it to 10 miles of 3:15water watching carefully 3:33and we're still watching you'll notice 3:37this one is taking a little bit longer 3:39now from the first experiment what we 3:48notice is that concentration affects the 3:52rate of a reaction remember please any 3:55calculations that you do or graphs that 3:58you make 3:58please show all of your work thank you 4:01very much
Views: 6658 W CLN
Iodine Clock.
 
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It is amazing how the change is so dramatic and has no warning. The first solution is Potassium Iodate. The second solution is vinegar, starch, and sodium bisulfite. This video has no special effects and is done in real time. When Solutions A and B are mixed, the chemicals start reacting immediately but the reaction to produce the dark bluish-black iodine complex seems to take time and hence this is called a clock reaction. In the first step, the iodate ion from the potassium iodate solution reacts with the bisulfite ion to produce colorless iodide and colorless bisulfate ions. This is the slowest or rate determining step of the reaction: IO3- (aq) + 3HSO3- (aq) → I- (aq) + 3HSO4-(aq) The second step is when the iodate in excess will oxidize the iodide generated above to form iodine (I2). IO3- (aq) + 5I- (aq) + 6H+ (aq) → 3I2 + 3H2O (l) Iodine is usually yellow-orange in color but in the presence of starch and excess iodide ion, the tri-iodine ion starch complex is formed which is bluish-black in color. The third reaction step are shown here and in the diagram in the top right: 3I2 + I-1 → I3-1 The reason there is a delay in color change in this chemical reaction is a fourth step occurs where the iodine is reduced immediately back to colorless iodide (I-1) by the bisulfite: I2 (aq) + HSO3- (aq) + H2O (l) → 2I- (aq) + HSO4-(aq) + 2H+ (aq) Only a small amount of bisulfite was used in this reaction so when the bisulphite is fully consumed, the iodine no longer reduced to colorless iodide so in an instant the dark blue complex with starch is formed producing the sudden color change but with a delayed reaction from the initial mixing.
Views: 27 Loran Krysl
Iodine Clock Teamwork
 
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Student groups were assigned varying molarities (0.046M to 0.018M) of potassium iodate to vary the reaction rate of the iodine clock. The other solution was a mix of water, starch, sulfuric acid and sodium bisulfite. Solution B is a complex solution of water, 10 seconds of liquid starch, 2.0 mL of 18M concentrated H2SO4 with 0.80 g of sodium bisulfite (NaHSO3) in 2000.0 mL of total solution volume. When the bisulfite ion is consumed, the reaction suddenly changes color because of the build up of triiodide Ion in the starch complex. When Solutions A and B are mixed, the chemicals start reacting immediately but the reaction to produce the dark bluish-black iodine complex seems to take time and hence this is called a clock reaction. In the first step, the iodate ion from the potassium iodate solution reacts with the bisulfite ion to produce colorless iodide and colorless bisulfate ions. This is the slowest or rate determining step of the reaction: IO3- (aq) + 3HSO3- (aq) → I- (aq) + 3HSO4-(aq) The second step is when the iodate in excess will oxidize the iodide generated above to form iodine (I2). IO3- (aq) + 5I- (aq) + 6H+ (aq) → 3I2 + 3H2O (l) Iodine is usually yellow-orange in color but in the presence of starch and excess iodide ion, the tri-iodine ion starch complex is formed which is bluish-black in color. The third reaction step are shown here and in the diagram in the top right: 3I2 + I-1 → I3-1 The reason there is a delay in color change in this chemical reaction is a fourth step occurs where the iodine is reduced immediately back to colorless iodide (I-1) by the bisulfite: I2 (aq) + HSO3- (aq) + H2O (l) → 2I- (aq) + HSO4-(aq) + 2H+ (aq) Only a small amount of bisulfite was used in this reaction so when the bisulphite is fully consumed, the iodine no longer reduced to colorless iodide so in an instant the dark blue complex with starch is formed producing the sudden color change but with a delayed reaction from the initial mixing. For other cool iodine clock reactions, check out these YouTube vidoes: https://www.youtube.com/watch?v=zTakExx4Buw https://www.youtube.com/watch?v=UJV04umAb6w&t=12s https://www.youtube.com/watch?v=Tv6_IsdnaGg
Views: 38 Loran Krysl
Iodine and Starch Experiment | Iodine Experiment | Starch Experiment | Science experiments for kids
 
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Iodine and Starch Experiment | Iodine Experiment | Starch Experiment | Science experiments for kids Simple and easy experiment to demonstrate the iodine with starch reaction! For this test you will need: • Two test tubes • Soluble starch powder • Iodine solution • Water • Dropper Procedure: • Put some starch powder into a test tube and fill the test tube with water. • Mix the starch in the test tube well until the starch dissolves in the water. • Fill the other test tube with normal water. • Place both the test tubes in a test tube stand. • Using a dropper take iodine solution. • Put some drops in each test tube. • Observe that the test tube with starch solution turns to purple black color. • The other test tube with normal water retains the color of iodine i.e orange or yellow. Explanation: Starch is a mixture of amylose and amylopectin, which are different forms of glucose/starch. Amylose in starch is responsible for the formation of a deep blue black color. Amylase is long polymer chains of glucose units connected by an alpha acetal linkage and looks much like a coiled spring. However iodine is a potassium iodide reagent and it is not very soluble in water. So, iodine is prepared by dissolving it in water in an aqueous solution of potassium iodide. This results in a linear tri-iodide ion (I3−) complex in iodine which is soluble. This tri-iodide ion (I3−) slips into the coil of the starch causing an intense or deep blue-black color.
Views: 179008 Elearnin
Clock Reaction Part 3
 
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Describes the procedures for each part in the Clock Reaction Lab
Views: 1937 Sehat Nauli
Chemical Kinetics 3
 
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Chemical Kinetics Lab
Views: 148 doughboi734
AP Chemistry Lab- Kinetics
 
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Kinetics, woo!
Views: 742 Elaine Moore
Chemical Kinetics - Reaction rates
 
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Reaction rates with change in temperature
Views: 6773 Yuriy Y.
IB Chemistry on Kinetics experiments and Rate of chemical reaction for IA design
 
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IB Chemistry on Kinetics experiments and Rate of chemical reaction for IA design
Views: 4269 wkkok1957
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: 8750 drbodwin
Monitoring Reaction Rates - Chemistry 12 - Sec 1.2
 
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Section 1.2 - Monitoring Reaction Rates In this video, a variety of ways to monitor reaction rate will be discussed. Temperature changes, volume and pressure changes, mass changes and concentration of aqueous ions. Also, the difference between homogeneous and heterogeneous reactions will be defined.
Views: 3909 Arcuricacid
Kinetics Demo
 
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Views: 61 Rast Chem
Clock reaction / Temperature 1 (70 C)
 
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The reaction started out at 70C (not 72C as indicated on the label in the video) and it was cooling quite rapidly. The clock reaction used is the potassium iodide / potassium persulfate reaction as listed on CLEAPSS Recipe booklet RB29. 5ml solution A, sodium thiosulfate & starch 50ml solution B, potassium persulfate 50ml solution C, 0.1M potassium iodide Mix solutions A then B then C in that order and start timing until it turns dark blue. Further details about the reaction are quite easy to find by doing a web search. From the CLEAPSS recipe booklet RB29 the stock solutions are made up as follows: "Solution A Dissolve 0.25 g of sodium thiosulfate in 100 ml of 1% starch solution. Solution B Dissolve 13.50 g of potassium persulfate in 1000 ml of solution. Solution C 0.1 M potassium iodide. Mix 5 ml of solution A with 50 ml each of solutions B and C in that order."
Views: 381 Nigel Baldwin
Colorimetry
 
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A look at how colorimetry is used to continuously monitor the rate of a chemical reaction
Views: 4507 MaChemGuy
ChemLab - 9. Kinetic Study of the Reaction between Ferric and Iodide Ions
 
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Middle East Technical University OpenCourseWare [ http://ocw.metu.edu.tr ] Chemistry Department 9. Kinetic Study of the Reaction between Ferric and Iodide Ions Course Link: http://ocw.metu.edu.tr/course/view.php?id=99
Views: 2139 METUOpenCourseWare
Reaction Rates Part 1.m4v
 
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Part 2 of the reaction rate lab.
Views: 424 rjgraziani
Sudsy Kinetics
 
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Take advantage of the overflowing fun in the "Old Foamy" reaction of hydrogen peroxide to teach students about the effect of concentration and the role of a catalyst on the rate of a chemical reaction. 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: 1648 FlinnScientific
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

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