logging in or signing up Equilibrium and le Chatelier's Principle pwict Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 36 Category: Education License: Some Rights Reserved Like it (0) Dislike it (0) Added: July 31, 2011 This Presentation is Public Favorites: 0 Presentation Description Introduction for Year 12 Research Assignment Comments Posting comment... Premium member Presentation Transcript Chemical Equilibrium: Chemical Equilibrium Reversible Reactions Chapter 17Equilibrium: Equilibrium Equal? Stable? Balance? . =Imagine – isolated zone – just Aus & NZ - No migration: Imagine – isolated zone – just Aus & NZ - No migrationPopulation of Australia 20,600,900 Population of New Zealand 4,173,460: Population of Australia 20,600,900 Population of New Zealand 4,173,460 Equilibrium StaticPopulation of Australia 20,600,900 Population of New Zealand 4,173,460: Population of Australia 20,600,900 Population of New Zealand 4,173,460 Equilibrium Dynamic 20,000 pa 20,000 paPopulation of Australia 15,000,000 Population of New Zealand 3,000,000: Population of Australia 15,000,000 Population of New Zealand 3,000,000 Equilibrium Not in 5,000 pa 20,000 paPopulation of Australia 18,000,000 Population of New Zealand 3,000,000: Population of Australia 18,000,000 Population of New Zealand 3,000,000 Equilibrium Not in 20,000 pa 10,000 paEquilibrium populations remaining constant: Equilibrium populations remaining constant Equilibrium Dynamic same same More importantVapours above Liquids: Vapours above Liquids CH 3 CH 2 OH (l) CH 3 CH 2 OH (g) CH 3 CH 2 OH (l)Rate Graph: Rate Graph Time Rate Rate of evaporation Rate of condensationEquilibrium Constant: Equilibrium Constant N 2(g) + 3H 2(g) 2 NH 3(g) N 2(g) + H 2(g ) + H 2(g ) + H 2(g) NH 3(g) + NH 3(g ) K = [NH 3 ] [NH 3 ] [N 2 ] [H 2 ] [H 2 ] [ H 2 ] K = [NH 3 ] 2 [N 2 ] [ H 2 ] 3Equilibrium Constant: Equilibrium Constant aA + bB + cC zZ + yY + xX (a moles of A etc ) K = [Z] z [Y] y [X] x [A] a [B] b [C] c Size of K: High – little reactant remaining at equilibrium Low – little product formed at equilibrium Calculations p 566 - 570Changing Equilibrium Constant: Changing Equilibrium Constant Rigging it to get what we wantEquilibrium example: Equilibrium example Equilibrium DynamicLe Chatelier’s Principle: Le Chatelier’s Principle Any change that affects the position of an equilibrium, will cause the equilibrium to shift, if possible, in such as way as to oppose the effect of that change. Examples You make it hotter? Favours an endothermic reaction You increase the pressure? Favours the arrangement with less pressure. Opposite!Temperature: Temperature N 2(g) + 3H 2(g) 2 NH 3(g ) H = -46kJ kJ/ mol Exothermic – forward reaction make it hot Reduce temperature – favours this reaction Increase temperature – favours reverse reactionPressure: Pressure Avogadro’s hypothesis: Equal volumes of gases (at the same pressure and temperature) contain the same number of molecules. Never mind the size of the molecules. n determines VPressure: Pressure N 2(g) + 3H 2(g) 2 NH 3(g ) H = -46kJ kJ/ mol Volume of a gas depends on n n for left side? 4 n for right side? 2 Increase pressure– favours forward reaction Decrease pressure– favours reverse reactionConcentration: Concentration N 2(g) + 3H 2(g) 2 NH 3(g ) H = -46kJ kJ/ mol Pump in more N 2(g) Favours forward reaction Pump in more NH 3(g ) Favours reverse reaction Pump in more H 2(g ) Favours forward reactionDilemma – chemical manufacturing: Dilemma – chemical manufacturing Manipulate factors to obtain the highest equilibrium constant Improve yield Problems? Expensive equipment C onflict with reaction rates You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
Equilibrium and le Chatelier's Principle pwict Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 36 Category: Education License: Some Rights Reserved Like it (0) Dislike it (0) Added: July 31, 2011 This Presentation is Public Favorites: 0 Presentation Description Introduction for Year 12 Research Assignment Comments Posting comment... Premium member Presentation Transcript Chemical Equilibrium: Chemical Equilibrium Reversible Reactions Chapter 17Equilibrium: Equilibrium Equal? Stable? Balance? . =Imagine – isolated zone – just Aus & NZ - No migration: Imagine – isolated zone – just Aus & NZ - No migrationPopulation of Australia 20,600,900 Population of New Zealand 4,173,460: Population of Australia 20,600,900 Population of New Zealand 4,173,460 Equilibrium StaticPopulation of Australia 20,600,900 Population of New Zealand 4,173,460: Population of Australia 20,600,900 Population of New Zealand 4,173,460 Equilibrium Dynamic 20,000 pa 20,000 paPopulation of Australia 15,000,000 Population of New Zealand 3,000,000: Population of Australia 15,000,000 Population of New Zealand 3,000,000 Equilibrium Not in 5,000 pa 20,000 paPopulation of Australia 18,000,000 Population of New Zealand 3,000,000: Population of Australia 18,000,000 Population of New Zealand 3,000,000 Equilibrium Not in 20,000 pa 10,000 paEquilibrium populations remaining constant: Equilibrium populations remaining constant Equilibrium Dynamic same same More importantVapours above Liquids: Vapours above Liquids CH 3 CH 2 OH (l) CH 3 CH 2 OH (g) CH 3 CH 2 OH (l)Rate Graph: Rate Graph Time Rate Rate of evaporation Rate of condensationEquilibrium Constant: Equilibrium Constant N 2(g) + 3H 2(g) 2 NH 3(g) N 2(g) + H 2(g ) + H 2(g ) + H 2(g) NH 3(g) + NH 3(g ) K = [NH 3 ] [NH 3 ] [N 2 ] [H 2 ] [H 2 ] [ H 2 ] K = [NH 3 ] 2 [N 2 ] [ H 2 ] 3Equilibrium Constant: Equilibrium Constant aA + bB + cC zZ + yY + xX (a moles of A etc ) K = [Z] z [Y] y [X] x [A] a [B] b [C] c Size of K: High – little reactant remaining at equilibrium Low – little product formed at equilibrium Calculations p 566 - 570Changing Equilibrium Constant: Changing Equilibrium Constant Rigging it to get what we wantEquilibrium example: Equilibrium example Equilibrium DynamicLe Chatelier’s Principle: Le Chatelier’s Principle Any change that affects the position of an equilibrium, will cause the equilibrium to shift, if possible, in such as way as to oppose the effect of that change. Examples You make it hotter? Favours an endothermic reaction You increase the pressure? Favours the arrangement with less pressure. Opposite!Temperature: Temperature N 2(g) + 3H 2(g) 2 NH 3(g ) H = -46kJ kJ/ mol Exothermic – forward reaction make it hot Reduce temperature – favours this reaction Increase temperature – favours reverse reactionPressure: Pressure Avogadro’s hypothesis: Equal volumes of gases (at the same pressure and temperature) contain the same number of molecules. Never mind the size of the molecules. n determines VPressure: Pressure N 2(g) + 3H 2(g) 2 NH 3(g ) H = -46kJ kJ/ mol Volume of a gas depends on n n for left side? 4 n for right side? 2 Increase pressure– favours forward reaction Decrease pressure– favours reverse reactionConcentration: Concentration N 2(g) + 3H 2(g) 2 NH 3(g ) H = -46kJ kJ/ mol Pump in more N 2(g) Favours forward reaction Pump in more NH 3(g ) Favours reverse reaction Pump in more H 2(g ) Favours forward reactionDilemma – chemical manufacturing: Dilemma – chemical manufacturing Manipulate factors to obtain the highest equilibrium constant Improve yield Problems? Expensive equipment C onflict with reaction rates