Stephany Matos Chem Lab: Chemical Equilibrium Lab 52 Synopsis Iron (III) ions react with thiocyanate ions (SCN-) to form iron (III) thiocyanate‚ FeSCN2+. It is represented in the equation below: Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq) Therefor the equilibrium constant for this reaction is: KC = [FeSCN2+]/([Fe3+]•[SCN-] For this experiment we were able to determine the equilibrium constant KC for this reaction. First we prepared five different mixtures with known initial concentrations of
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CHM 096 TUTORIAL 2 (Chemical Equilibrium) 1. Write the equilibrium constant expression‚ Kc‚ for each of the following reactions: a) 2NO(g) + O2(g) ⇄ 2NO2(g) b) The decomposition of solid potassium chlorate to solid potassium chloride and oxygen gas. c) 4HCl(g) + O2(g) ⇄ 2H2O(g) + 2Cl2(g) d) 2NO2(g) + 7H2(g) ⇄ 4H2O(l) + 2NH3(g) e) H2O(g) + C(s) ⇄ CO(g) + H2(g) f) The reduction of solid copper (II) oxide with hydrogen gas to produce copper metal and
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CHEMICAL EQUILIBRIUM I. Introduction In a chemical reaction‚ when reactants are mixed together in a reaction vessel‚ the whole of the reactants do not get converted into products. After some time‚ there will come a point when a fixed amount of reactants will exist in harmony with a fixed amount of products; neither amount will change anymore. This state is called chemical equilibrium (Birk‚ 1994; Jones‚ 1987; LeMay‚ 2002). There are three characteristics of a system in chemical equilibrium: a
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9 CHEMICAL EQUILIBRIUM Audrey De Castro FCD3‚ Group 9‚ Ms. Sarah Sibug Kristine Tavares March 27‚ 2014 I. ABSTRACT Chemical equilibrium is mostly involved in industrial processes such as synthesis of ammonia
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1. Briefly explain the following: a. Chemical equilibrium- Chemical equilibrium is the state of a reaction when the concentrations of the reactants and products are no longer changing and remain constant. The forward reaction proceeds at the same rate as the reverse reactions making them equal. This type of equilibrium is also named dynamic equilibrium or a dynamic process. When a reaction has reached its chemical equilibrium‚ the constant K value will remain constant unless the temperature changes
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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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Chemical Equilibrium: Le Châtelier’s Principle Abstract This experiment entitled "Chemical Equilibrium" aims to help students to investigate the effects of concentration and temperature upon the position of equilibrium in a cobalt chloride solution‚ Co(H2O)62+. In this experiment‚ cobalt crystal is dissolved with distilled water and ethanol which the initial colour is purple-pinkish and a few drops of concentration of HCl is added to the test tube‚ the final colour is in deep blue colour. Upon
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is considered in a state of equilibrium when its properties do not change at time passes. Equilibrium is a state of a reaction where the concentration of all the reactants and all the products remain constant over time. Equilibrium as used in chemical systems means that all the chemical forces in a reaction are in balance and that all physical properties of the system (color‚ density and concentration) of all chemicals species involved remains constant. The equilibrium state can be characterized by
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Ashley Silva Lab 7: Three Stooges in Chemical Reactions Objective: The purpose of this lab is to experimentally determine the equilibrium constant‚ Kc ‚ for the following chemical reaction: Fe3+ (aq) + SCN-(aq) ↔FeSCN2+(aq) Background Information: A system is at equilibrium when the rate of the forward reaction is the same as the rate of the reverse reaction. There is no change in concentration for the reactants or products at chemical equilibrium. When the system is disturbed there is
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Temperature to the reaction C. Effect of Concentration to the Reaction Rate D. Effect of Catalyst to the Reaction Rate E. Chromate-Dichromate Equilibrium F. Thiocyanatoiron (III) Complex Ion Equilibrium G. Weak Acid Equilibrium (Ionization of Acetic Acid) H. Weak Base Equilibrium Ionization of Ammonia I. Saturated Salt (Sodium Chloride) Equilibrium On part (A) we are to observe which reaction rate is faster‚ and doing the experiment. We have concluded that: “Aluminum had faster rate of reaction
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