www.economicshelp.org Micro Economic Essays Market Structure 1. Discuss how firms within an oligopolistic market compete. 2. Discuss whether monopoly is always an undesirable form of market structure. 3. Explain how interdependence and uncertainty affect the behaviour of firms in Oligopolistic markets 4. Evaluate the view that only producers‚ and not consumers‚ benefit when oligopolistic firms collude to try to reduce the uncertainty they experience. 5. Explain why contestable markets
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and answer these questions: A. Which way should the equilibrium shift when HCl is added? How do your results support your answer? It should shift to the left because adding any component causes the equilibrium to shift to the opposite side. B. Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer? It should shift to the right because the removal of a component causes the equilibrium to shift to the side from which the component was removed
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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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single or multivalued mappings is obtained as a corollary of Nash equilibrium existence in finitely many players games. ı Copyright © 2006 Juan Pablo Torres-Mart´nez. This is an open access article distributed under the Creative Commons Attribution License‚ which permits unrestricted use‚ distribution‚ and reproduction in any medium‚ provided the original work is properly cited. 1. Introduction In game theory‚ the existence of equilibrium was uniformly obtained by the application of a fixed point theorem
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Experiment 1: Study of Solubility Equilibrium Data Treatment and Analysis Section 1: Solubility Product Constant Temperature (˚C) | Volume of NaOH used (mL) | | | | Titration 1 | Titration 2 | Average | 28 | 12.7 | 12.8 | 12.75 | 9 | 10.5 | 10.5 | 10.5 | 19 | 11.3 | 11.2 | 11.25 | 40 | 16.2 | 16.2 | 16.2 | 50 | 22.8 | 22.9 | 22.85 | Table 1: The volume of NaOH used in the titration at various temperatures. No. of moles of KHC4H4O6 = 1.45 g ÷ 188.177g/mol = 7.71 x 10-3mol
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CHAPTER 3 The Competitive Environment Learning Objectives Upon completing this chapter‚ you should be able to: Identify the structural characteristics of the environment faced by the firm and how these drivers influence both competition and value creation Choose the appropriate level of specificity in environmental analysis‚ depending on the locus of the decision-making group Predict how changes occurring in the environment might influence future competition and value creation Incorporate understanding
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Determination of Equilibrium Constants Introduction Bromothymol blue is an indicator for many acid-base titrations. When adding different solutions within the indicator it is to react and change colors‚ in this experiment the different colors were blue‚ green‚ and yellow. In the following experiment‚ obtaining the absorbance levels for each one makes it possible to calculate the equilibrium constant. Materials and Methods For this specific experiment there are a few materials that are crucial
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CHM 096 TUTORIAL 2 (Chemical Equilibrium) Jan 2013 1. Write the equilibrium constant expression‚ Kc‚ for each of the following reactions: a) b) c) d) e) f) 2NO(g) + O2(g) ⇄ 2NO2(g) The decomposition of solid potassium chlorate to solid potassium chloride and oxygen gas. 4HCl(g) + O2(g) ⇄ 2H2O(g) + 2Cl2(g) 2NO2(g) + 7H2(g) ⇄ 4H2O(l) + 2NH3(g) H2O(g) + C(s) ⇄ CO(g) + H2(g) The reduction of solid copper (II) oxide with hydrogen gas to produce copper metal and water at o 500 C. 2H2(g) + O2(g)
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Introduction: Chemical equilibrium is when the concentrations of the reactants and products have reached a state where reactions occurring in one direction are at the same rate of reactions occurring in the opposite direction. This process‚ called dynamic equilibrium‚ is the main subject of Le Chatelier’s Principle. Le Chatelier pointed out that if a system at equilibrium is subjected to a stress that momentarily causes the system to be not in equilibrium‚ a spontaneous change will occur to
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DISCUSSION Chemical equilibrium and its different applications were studied in this experiment. The Le Chatelier’s principle‚ which is the main principle behind chemical equilibrium‚ states that‚ “If an external stress is applied to a system at equilibrium‚ the system adjusts in such a way that the stree is partially offset as the system reaches a new equilibrium position.”[1] The “stress” can be a change in concentration‚ volume‚ pressure‚ or temperature that disturbs the equilibrium
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