the equilibrium constant from pH values of changing concentrations of ethanoic acid Design Research question: How will altering the concentrations of ethanoic acid affect the pH value‚ and‚ in-turn‚ the equilibrium constant? Background information: When weak acids react‚ the reaction typically does not go to completion. Rather‚ the system goes to an intermediate state in which the rates of the forward and reverse reactions are equal. Such a system is said to be in chemical equilibrium. When
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Problem: For the reaction H2(g) + I2(g) ↔ 2 HI(g) At equilibrium‚ the concentrations are found to be [H2] = 0.106 M [I2] = 0.035 M [HI] = 1.29 M What is the equilibrium constant of this reaction? Solution The equilibrium constant (K) for the chemical equation aA + bB ↔ cC + dD can be expressed by the concentrations of A‚B‚C and D at equilibrium by the equation K = [C]c[D]d/[A]a[B]b For this equation‚ there is no dD so it is left out of the equation. K = [C]c/[A]a[B]b
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TOPIC 1: RATES AND CHEMICAL EQUILIBRIUM QUESTION 1: (Taken from the DoE Physical Sciences Feb-March Paper 2 2009) Antacids are used to relieve indigestion. Indigestion is the condition when the stomach produces too much acid resulting in an uncomfortable and painful feeling. A certain antacid tablet dissolves in water and reacts with the acid in the stomach to release carbon dioxide gas. 1.1 Name the type of chemical reaction that explains why antacids bring relief from indigestion
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EXPERIMENT NO. 4 Chemical Equilibrium Claver‚ L. Z. X. Y.1‚ Palad‚ C. C.2‚ Rocha‚ R. D. P3 1Anthropology Department‚ College of Social Sciences and Philosophy‚ 2National Institute of Geological Sciences‚ College of Science‚ 3Department of Food Science and Nutrition‚ College of Home Economics‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines ------------------------------------------------- Keywords: forward and reverse reactions‚ equilibrium constant‚ Le Chatelier’s Principle
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Objectives * To determine the equilibrium constant for a given reaction * To understand the concept of Le Chatelier’s Principle * To gain experience in the use of a UV Spectrophotometer Background/Concepts * A chemical equilibrium is the state reached by a reaction mixture when the forward reaction and the reverse reaction occur at equal rate‚ resulting in constant values for the concentrations of the reactants and products. * The equilibrium constant Kc for a reversible reaction
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1) At equilibrium‚ __________. A) all chemical reactions have ceased B) the rate constants of the forward and reverse reactions are equal C) the rates of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed 2) Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (s) + H2O (l) ⇌ H3O+ (aq) + F- (aq) A) [HF][H2O] / [H3O+][F-] B) 1 /[HF]
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purpose of this experiment is to understand the components of a reaction at chemical equilibrium and use Le Chatelier’s principle to predict the direction an equilibrium position will shift upon changes in the concentration‚ temperature‚ and pressure. It was determined that in the equilibrium of chromate and dichromate it is an exothermic reaction and in the equilibrium of ferrocyanide and ferric ferrocyanide that it is an equilibrium shift to the left after adding NaOH. Experiment and Observation: The
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SPECTROPHOTOMETRIC DETERMINATION OF THE EQUILIBRIUM CONSTANT OF A REACTION M. L. SANGA CHEMICAL ENGINEERING‚ COLLEGE OF ENGINEERING UNIVERSITY OF THE PHILIPPINES‚ DILIMAN‚ QUEZON CITY‚ PHILIPPINES DATE PERFORMED: JANUARY 15‚ 2014 INSTRUCTOR’S NAME: MOISES JEROME GARRERO ______________________________________________________________________________________________________________________________ ABSTRACT The experiment aimed to determine the equilibrium constant Keq of the formation of Fe(SCN)2+
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participants: [List names] Section Number: [List 3-digit number] Meeting Time: [Fill in the lab meeting time] TA: [Fill in the lab TA’s name] INTRODUCTION In this experiment I calculated the equilibrium constant for the reaction shown below under different conditions to determine if the equilibrium constant is really constant. Fe3+ (aq) + SCN– (aq) ←→ FeSCN2+ (aq) A big part of this lab includes understanding (and in the end proving) that absorbance is directly proportional to the concentration
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Determination of the Equilibrium Constant of an Unknown Ester Hydrolysis Reaction Abstract The experiments to follow determined that the equilibrium concentrations of the reaction: ester + water ↔ alcohol + acid‚ are equal to 0.0363 moles of ester‚ 0.2852 moles of water‚ and 0.0268 moles each of alcohol and acid. Using this information the equilibrium constant was determined to be 0.06938. 1. Introduction In this lab the equilibrium constant‚ Kc‚ for the acid catalyzed reaction
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