christinaT87 Posted February 2, 2005 Report Share Posted February 2, 2005 Can you please help me understand my homework? This is about Le Chateliers principle... I have this equilibrium reaction: CO(g) + H2O <---> CO2(g) + H2 (g) + energy In which direction will the reaction go if you: 1) increase pressure? 2) increase temperature? thank youu Quote Link to comment Share on other sites More sharing options...
Tim_Lou Posted February 2, 2005 Report Share Posted February 2, 2005 1) well, it depends on the state of H2O, is it in gasous state? or liquid?if it is vapor, increseing pressure will not affect the equilibrium, since both side have the same amout of molecules.if it is in liquid state, incresing pressure will shift the equilibrium to the left, since increasing pressure favors a lesser volume.(i doubt that H2O is in liquid state though, since CO2 will establish another equilibrium with water and forms H2CO3... :hyper: ) 2) increasing temperature will increase the kinetic energy of the system, which can be counted as one of the "product", thus the equilbrium will shift to the left. Quote Link to comment Share on other sites More sharing options...
Fishteacher73 Posted February 2, 2005 Report Share Posted February 2, 2005 2) increasing temperature will increase the kinetic energy of the system, which can be counted as one of the "product", thus the equilbrium will shift to the left. Would not pressure also be a form of energy and thus push the equilibrium to the left as well? Quote Link to comment Share on other sites More sharing options...
Tim_Lou Posted February 3, 2005 Report Share Posted February 3, 2005 pressure is not energy, it is force per area.edit: the explanation i gave in this post before is totally irrelevant. Quote Link to comment Share on other sites More sharing options...
sciencegirl07 Posted June 2, 2008 Report Share Posted June 2, 2008 assuming H2O is gaseous pressure would have no effect on the equilibrium, since pressure affects gaseous systems only where one side has less molecules than the other (equilibrium would shift to the side of the reaction where there are less molecules).temperature increase=increase in average kinetic energy=equilibrium shift left, since the reaction is exothermic, and le chatelier's principle states that a chemical reaction will resist changes to its state of equilibrium (if i remember correctly). Quote Link to comment Share on other sites More sharing options...
modest Posted June 2, 2008 Report Share Posted June 2, 2008 I agree with Tim_Lou. Also, if you haven't got into calculating equilibrium constants yet - but are just looking at Le Chatelier's Principle conceptually, this should be a really good site: Le Chatelier's Principle -modest //editOne thing the site above does not note, but which will help you is that: If energy is stated on the left side or reactants side of the equation then it should be taken as an endothermic reaction. If it is on the right side with the products it is an exothermic reaction. Quote Link to comment Share on other sites More sharing options...
C1ay Posted June 2, 2008 Report Share Posted June 2, 2008 You do realize this discussion is from 3 years ago..... Quote Link to comment Share on other sites More sharing options...
modest Posted June 2, 2008 Report Share Posted June 2, 2008 You do realize this discussion is from 3 years ago..... I know, I've been working on this one for a really long time :) Quote Link to comment Share on other sites More sharing options...
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