LE CHATELIER’S PRINCIPLE Castro‚ Lharize C. Experiment # 1 I. Introduction: In this experiment‚ using Le Chatelier’s principle‚ we will observe several responses of a system at equilibrium to various changes in external conditions. The experiment aims to investigate two equilibrium systems: (a) cobalt complexes and (b) chromate-dichromate equilibrium and explain observations in light of the Le Chatelier’s principle. II. Theory/Concepts: In 1884 the French chemist and engineer Henry-Louis
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Chapter 4 Fundamentals of Material Balances Material Balance-Part 1 Process Classification 3 type of chemical processes: 1. Batch process – Feed is charge to the process and product is removed when the process is completed – No mass is fed or removed from the process during the operation – Used for small scale production – Operate in unsteady state March 31‚ 2009 ChE 201/shoukat@buet.ac.bd 2 Process Classification 2. Continuous process – Input and output is continuously
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Involving Chromate and Dichromate Ions Steps 2 and 3 0.1 M K2CrO4 0.1 M K2Cr2O7 Initial Color 1 M NaOH added 1 M HCl added Step 4 0.1 M K2CrO4 0.1 M K2Cr2O7 Initial Color 1 M HCl added 1 M NaOH added Steps 5 and 6 INITIAL COLOR + 1 M NaOH + 0.1 M Ba(NO3)2 + 1 M HCl 0.1 M K2CrO4 Steps 7 and 8 INITIAL COLOR + 1 M HCl + 0.1 M Ba(NO3)2 + 1 M NaOH 0.1 M K2Cr2O7 Step 9 0.1 M K2CrO4 0.1 M K2Cr2O7 Add 0.1 M Ba(NO3)2 Table 5 Equilibrium
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Name ___________________________________________ Date ___________________________________ Block ____ Experiment 12A Investigating chemical equilibrium ABSTRACT 1. What is equilibrium and how can you tell it has been reached? __________________________________________________________________________________________ __________________________________________________________________________________________ __________________________________________________________________________________________
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1. | An experiment is carried out to determine the freezing point of naphthalene.Solid naphthalene is heated in a water bath until it melts completely. The initial temperature is recorded. Then molten naphthalene is left to cool. The reading of the temperature is recorded every 30 seconds. Figure below shows the recorded thermometer readings at 30 seconds intervals. Satu eksperimen dijalankan untuk menentukan takat beku naftalena. Pepejal naftalena dipanaskan di dalam kukus air sehingga melebur
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Investigating Chemical Equilibrium Date: 30th April 2013 Due Date: 15th May 2013 Prepared For: M. Seraji Prepared by: Andrea Odunze Abstract Many reactions proceed to a state of equilibrium. A chemical reaction at equilibrium‚ where the rates of the forward reaction and reverse reaction are equal‚ looks like this: A + B AB There are three factors‚ according to Le Chatelier’s principle‚ that affect the equilibrium position and equilibrium constant. These are the concentrations of products
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sparker 2 -250mL beakers 10mL grad cylinder 0.2M FeCl3 0.2M KSCN 0.2M KCl 0.2M Fe(NO3)3 6.0M NaOH CoCl26H2O 6.0M HCl water 0.1M K2CrO4 0.1M K2Cr2O7 1M NaOH 1M HCl 0.1M Ba(NO3)2 Procedure PART I 1. Use a 10mL graduated cylinder to measure 1mL of 0.2M FeCl3 and pour it into a 250mL beaker. Using another 10mL graduated cylinder‚ measure
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using stoichiometry. II. Materials: * 0.00500 moles of potassium chromate * 0.00500 moles of lead (II) nitrate III. Procedures/ Observations: IV. Observation & Data Balanced Equation: K2CrO4 + Pb(NO3)2 2KNO3 + PbCrO4 Mass of lead (II) nitrate used: 0.00500 mol Pb(NO3)2 × 331.2 g PbNO 1 mol Pb(NO ) = 1.7 g Pb(NO3)2 Mass of potassium chromate used: 0.00500 mol
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Chemistry 12 - Lab 19A Flow Chart (Investigating Chemical Equilibrium) PART 1: Put on safety goggles and lab apron Obtain 2 (Empty‚ Clean‚ AND DRY) 250mL Erlenmeyer flasks. Add approx. 100mL of DISTILLED water and 1mL of thymol blue solution to each flask Record the colour of this solution in note book FIRST FLASK: add a single drop of 0.1M HCl. Swirl the contents of the flask and continue drop-by-drop addition until a definite colour change is observed. SECOND FLASK: will serve as
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Carlie Haeffner Qualitative Analysis March 20‚ 2015 The purpose of this lab is to identify unknown ions in a solution by using a type of chemical reaction called precipitate reactions. The key to finding which ions are present in a solution is to form a precipitate which makes the ions “come out” in a reaction (McNeil‚ 2013-2014). Water is used in these experiments to act as a solvent. Since water is a polar molecule‚ the slightly positive and negative charges will sometimes pull apart molecules
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