Composit ion 0613mo l 3h2g ch4g 1839mo l 0387mo

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Unformatted text preview: 13 = 0.1562 2 reject (concentration cannot be negat ive) correct Equilibrium Concentrations are: [PCl5] = 1.00 M – x = 1.00 M ­ 0.1351 M = 0.86 M [PCl3] = [Cl2] = x = 0.135 M Example 7: Calculate the composit ion of the gaseous mixture obtained when 1.25 mo l of carbon dioxide is exposed to hot carbon at 800 °C in a 1.25­L vessel. The equilibrium constant K at 800 °C is 14.0 c for the reaction: CO2 (g) ¾¾ ® + C (s) ¬¾ ¾ Init ial D Equilibrium [CO2] = Kc = 14.0 = 21 2 Cl (g) Chemistry 102 Chapter 14 LE CHATELIER’S PRINCIPLE · The effect of changes on the equilibrium can be predicted using the Le Chatelier’s principle. · Le Chatelier’s principle states that: “If a stress is applied to a system at equilibrium, the system will respond in such a way as to relieve the stress and restore a new equilibrium under a new set of condit ions”. · Note sequence of events: 1. Stress applied 2. Equilibrium system response (equilibrium shift) 3. New equilibrium · Stress is a change in any of the fo llowing: A) Concentration of Reactants or Products B) Pressure C) Temperature A) Effect of Concentration Change on Equilibrium (Adding or Removing Reactants or Products) Consider: A + Stress: B ¾¾ ® ¬¾ ¾ C + D increased to B* Response: Ø Forward reaction speeds up Ø Equilibrium shifts to the right Ø Products are favored...
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This document was uploaded on 03/18/2014 for the course CHEM 102 at Los Angeles Mission College.

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