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Search results “Determining the rate constant k from data”

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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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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: 310375 chemistNATE

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Views: 9502 Melissa Maribel

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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: 116914 SlowChem

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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: 48518 Michel van Biezen

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webpage-http://www.kentchemistry.com/aplinks/chapters/12ChemEq/rateconstantunits.htm This short video show you how to determine the units for a rate constant for zero (0th), first (1st), second (2nd) and third (3rd) order rate laws.
Views: 51948 kentchemistry.com

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More free chemistry help videos: http://www.chemistnate.com How to find the reaction order if you're given a table of kinetic data. Trick: Create two new columns, ln[A] (1st order) and 1/[A] (2nd order), then calculate first differences. Whichever set of first differences is approximately constant .... that corresponds to the order of your reaction.
Views: 165303 chemistNATE

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037 - The Rate Constant In this video Paul Andersen describes the characteristics of the rate constant in chemical reactions. The rate constant is highly variable in reactions and must be determined experimentally. The rate constant is dependent on both temperature and the presence of a catalyst. In a first-order reaction the rate constant and the half-life are both independent of the concentration and inversely proportional. 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:Aufgeschnittener Metall Katalysator Für Ein Auto.jpg." Wikipedia, the Free Encyclopedia. Accessed October 20, 2013. http://en.wikipedia.org/wiki/File:Aufgeschnittener_Metall_Katalysator_f%C3%BCr_ein_Auto.jpg. File:Thermometer 0.svg, n.d. http://commons.wikimedia.org/wiki/File:Thermometer_0.svg. "File:Verbrennung Eines Zuckerwürfels .png." Wikipedia, the Free Encyclopedia. Accessed October 19, 2013. http://en.wikipedia.org/wiki/File:Verbrennung_eines_Zuckerw%C3%BCrfels_.png. (n.d.). http://www.yorku.ca/tropchem/thesis/appdx-a.pdf.
Views: 107198 Bozeman Science

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Using Excel - Graphical Method
Views: 5181 Yu Kay Law

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Hi fellas!!! This is Chemaddicts again to the solution!! Today our topic is about Calculating Rate constant and Determining Mechanism of a reaction by rate equation Summary of this video tutorial: Today, in this tutorial, we'll learn about How to calculate the rate constant and determining the mechanism ? We will also discuss about building up the mechanism with help of the rate equation. We will discuss about: *The mark distribution of this question. *How to answer in the correct order? Finally we"ll discuss some of the keypoints of this problems... And that's all for today!!!!Enjoy this video tutoria!!! Thanks for reading this description.......:)

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Views: 597168 Brightstorm

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Sample concentration vs. time data is analyzed to determine the reaction order, rate law and rate constant.
Views: 27623 Eric Zuckerman

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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: 11532 LearnChemE

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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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For the following reaction: 2NO (g) + O2 (g) → 2NO2 (g) Determine the rate law from the given experimental data.

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Views: 20360 LPSChemistry

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This chemistry video tutorial provides the equations and formulas needed to solve zero order, first and second order integrated rate law problems including those with half life and rate constant K calculations. This video contains plenty of examples and practice problems for you to work on. Here is a list of topics: 1. Chemical Kinetics - Reaction Rates 2. Average Rate of Reaction Formula - Change in Concentration Divided By Change in Time 3. Concentration vs Time Graphs 4. Rate Law Expression - Rate Constant K and Initial Concentration 5. Zero Order Reaction - Integrated Rate Law Equation 6. Half Life Formula, Initial Concentration of Reactant and Rate Constant K Relationship 7. Units of Rate Constant K - Molarity, Moles, Liters, and Units of time - Seconds, Minutes, Hours, Days, etc 8. Inverse Relationship Between Rate Constant K and Half Life 9. Rate Constant K, Temperature, Activation Energy and Catalyst 10. Initial Rates vs Concentration 11. First Order Integrated Rate Law Equation 12. Straight line Plot - Ln[A] vs time - Graphs 13. Slope = -K Rate Constant 14. Half Life Independent of Initial Concentration for a first order reaction 15. Natural Log and Exponential Form of Integrated Rate Law 16. Second Order Reaction Integrated Rate Law Formula 17. Integrated Rate Law Problems 18. Identifying the Order of the Reaction Using the Units of K

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Average rate, determining ANY Rate Law from experimental data
Views: 16396 Michele Berkey

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✔ https://StudyForce.com ✔ https://Biology-Forums.com ✔ Ask questions here: https://Biology-Forums.com/index.php?board=33.0 Follow us: ▶ Facebook: https://facebook.com/StudyForcePS/ ▶ Instagram: https://instagram.com/studyforceonline/ ▶ Twitter: https://twitter.com/studyforceps Q1. Consider the reaction between nitrogen dioxide and carbon monoxide. NO2 (g) + CO (g) → NO (g) + CO2 (g) The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction Q2. Consider the following reaction: CHCl3 (g) + Cl2 (g) → CCl4 (g) + HCl (g) The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction ANALYSIS: Begin by examining how the rate changes for each change in concentration. Between the first two experiments, the concentration of NO2 doubles, the concentration of CO stays constant, and the rate quadruples, suggesting that the reaction is second order in NO2. Between the second and third experiments, the concentration of NO2 stays constant, the concentration of CO doubles, and the rate remains constant (the small change in the least significant figure is simply experimental error), suggesting that the reaction is zero order in CO. Between the third and fourth experiments, the concentration of NO2 again doubles, the concentration of CO halves, yet the rate quadruples again, confirming that the reaction is second order in NO2 and zero order in CO. Write the overall rate expression. ALTERNATIVE APPROACH If the relationships between the changes in concentrations and the changes in initial rates are not immediately obvious, you can determine the reaction order for any reactant by substituting any two initial rates and the corresponding initial concentrations into a ratio of the rate laws to determine the order (n). For NO2 use the first and second concentrations and rates (because [NO2] changes here, but [CO] is constant). Substitute the rates and concentrations into the expression for the ratio of the rate constants. Take the log of both sides of the equation and solve for n. For CO, use the second and third concentrations and rates (because [CO] changes here, but [NO2] is constant). Substitute the rates and concentrations into the expression for the ratio of the rate constants. Take the log of both sides of the equation and solve for n. Write the overall rate expression from the orders of each reactant. (b) To determine the rate constant for the reaction, solve the rate law for k and substitute the concentration and the initial rate from any one of the four measurements. In this case, you use the first measurement.
Views: 33 Study Force

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Practice Problems that determine the rate law from initial rate data. Solve for rate and rate constants.
Views: 2423 Linda Hanson

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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: 2174 Shawn Shields

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A tutorial on determining reaction orders and rate laws.

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Edited by Dan Rosenthal. Everything else by me.
Views: 104031 GenChem Concepts

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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: 2349 FranklyChemistry

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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: 26965 LearnChemE

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Views: 3984 Chem Lab

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Dr. Shields demonstrates how to determine the order of each reactant using a table of data collected in method of initial rates experiments. Part 1 of 3. General Chemistry
Views: 17468 Shawn Shields

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This chemistry video tutorial shows you how to write the rate law expressions and how to calculate the rate constant K with the appropriate units. It also provides the graphs and equations that correspond to a zero order, first order, and second order reaction. This video contains a few examples and practice problems. The half life formula and the rate law equations are also provided.

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This video is about Calculating the Rate Constant - Original

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Dr. Shields demonstrates how to calculate the value for the rate constant (with units) after determining the orders of each reactant using initial rates experimental data (done in part 1). Part 2 of 3. General Chemistry
Views: 27069 Shawn Shields

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Views: 4088 Tony St. John

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This tough nut to crack involves a rate table where concentration of reactants change on more than one reagent making it less obvious what effect that reagent has on rate. Take a look at this video to find out what I mean exactly. Hope this method will help!
Views: 26086 Allery Chemistry

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✔ https://StudyForce.com ✔ https://Biology-Forums.com ✔ Ask questions here: https://Biology-Forums.com/index.php?board=33.0 Follow us: ▶ Facebook: https://facebook.com/StudyForcePS/ ▶ Instagram: https://instagram.com/studyforceonline/ ▶ Twitter: https://twitter.com/studyforceps Q. Consider the equation for the decomposition of SO2Cl2. SO2Cl2 (g) → SO2 (g) + Cl2 (g) The concentration of SO2Cl2 is monitored at a fixed temperature as a function of time during the decomposition reaction, and the following data are tabulated: (a) Show that the reaction is first order and determine the rate constant for the reaction. (b) Use the graph and the best fitting line in the previous example to predict the concentration of SO2Cl2 at 1900 s. The First-Order Integrated Rate Law: Using Graphical Analysis of Reaction Data The plot is linear, confirming that the reaction is indeed first order. To obtain the rate constant, fit the data to a line. The slope of the line is equal to −k. Since the slope of the best fitting line (which is most easily determined on a graphing calculator or with spreadsheet software such as Microsoft Excel) is −2.90 × 10−4s−1, the rate constant is therefore +2.90 × 10−4s−1.
Views: 28 Study Force

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This chemistry video tutorial provides a basic introduction into reaction mechanisms within a chemical kinetics setting. It explains how to write the rate law expression for a reaction mechanism. A reaction mechanism consist of a series of elementary steps or elementary reactions whose rate law can be written from its molecularity - that is from the coefficients of the balanced reaction. The rate of a reaction mechanism is completely dependent on the slow step or the rate-determining step. This video explains how to substitute an intermediate when writing rate law expressions. 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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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: 2841 Real Chemistry

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Multiple experiments are run, varying the initial concentrations and measuring the rate. From the multiple experiments, we can solve for the exponents, and then the rate constant, k. this ends up being 1st order. 1st order equations are derived in this video.
Views: 7934 Michele Berkey

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This chemistry video tutorial provides a basic introduction into how to solve chemical equilibrium problems. It explains how to calculate the equilibrium constant k value given the equilibrium concentrations and equilibrium partial pressures of all reactants and products. If explains how to calculate the equilibrium constant k for a new reaction by changing another reaction. Finally, it discusses how to calculate the equilibrium constant k using ice tables. 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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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: 152060 Ben's Chem Videos

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IB Chemistry Topic 6 Kinetics 16.1 Rate expression and reaction mechanism Exploration of chemical kinetics using experimental data to determine reaction orders and mechanisms Full resources for topic 6: http://www.mrwengibchemistry.com/topic-6-kinetics.html 0:23 The rate equation 0:32 Order of reaction 1:13 Units for the rate constant k 2:26 Graphical determination of rate 2:46 Determining order with concentration vs time graph 3:45 Determining order with rate vs concentration graph 5:04 Rate of reaction calculations 6:12 Reaction mechanisms 8:17 Unimolecular vs bimolecular steps 8:59 Intermediate vs transition states 9:29 Enthalpy diagram: Intermediate vs transition states 10:05 Determining order of reaction from reaction mechanisms 11:26 Practice problems PPT direct link: https://mix.office.com/watch/1wzsr4ulr2s9u Free online Quiz SL: http://www.proprofs.com/quiz-school/story.php?title=NjAyODA3 Free onlin Quiz HL: http://www.proprofs.com/quiz-school/story.php?title=NjAyODI4 ​16.1 Rate expression and reaction mechanism HL • Reactions may occur by more than one step and the slowest step determines the rate of reaction (rate determining step/RDS). • The molecularity of an elementary step is the number of reactant particles taking part in that step. • The order of a reaction can be either integer or fractional in nature. The order of a reaction can describe, with respect to a reactant, the number of particles taking part in the rate-determining step. • Rate equations can only be determined experimentally. • The value of the rate constant (k) is affected by temperature and its units are determined from the overall order of the reaction. • Catalysts alter a reaction mechanism, introducing a step with lower activation energy. • Deduction of the rate expression for an equation from experimental data and solving problems involving the rate expression. • Sketching, identifying, and analysing graphical representations for zero, first and second order reactions. • Evaluation of proposed reaction mechanisms to be consistent with kinetic and stoichiometric data. Connect with me: Facebook: https://www.facebook.com/IBChemistry2016/ Twitter: https://twitter.com/andrewweng0406 Google plus: https://plus.google.com/u/0/108611113268141564345 Pinterest: https://www.pinterest.com/mrandrewweng040/ib-chemistry/
Views: 8564 Andrew Weng

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