1 / 11

Factors that Affect Equilibrium

Factors that Affect Equilibrium. Can an equilibrium constant be altered ?. What would happen if we changed The concentration of a reactant or product? The pressure of a reactant or product The t emperature of a system?. What would happen if we used a catalyst ?.

maegan
Download Presentation

Factors that Affect Equilibrium

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Factors that Affect Equilibrium • Can an equilibrium constant be altered ? • What would happen if we changed • The concentration of a reactant or product? • The pressure of a reactant or product • The temperature of a system? • What would happen if we used a catalyst? The position of the equilibrium of a system changes to minimise the effect of any imposed change on the system

  2. Concentration • Changing the concentration of a reactant or product will shift the position of an equilibrium to minimise the change CH3COOH (aq) + CH3CH2OH(aq) CH3COOCH2CH3(ag) + H2O(l) Increasing concentration of acid shifts equilibrium to the right, producing more ester & water Kc = [CH3COOCH2CH3] [H2O] [CH3COOH ][CH3CH2OH] Both the numerator & denominator increase Kc is the ratio of concentrations so… • Changing the concentration of a reactant or product will not affect the value of Kc

  3. Changing Pressure • Changing the pressure of a reactant or product will shift the position of an equilibrium to minimise the change N2(g) + 3H2(g) 2NH3(g) Increasing total pressure of the system shifts equilibrium to increasing the yield of ammonia Kp = (pNH3)2 (pN2)(H2)3 If total pressure has increased then the partial pressures of all the gases have also increased • Changing the pressure will not affect the value of Kp

  4. Changing Temperature • Changing the temperature of a system will shift the position of an equilibrium and will change the value of Kc or Kp. 2NH3(g) ∆H = -92kJmol-1 exothermic N2(g) + 3H2(g) Increasing temperature........... Favours backward reaction – trying to remove heat from system - equilibrium shifts to the left Decrease in yield of NH3 This term is reduced Kp = (pNH3)2 (pN2)(H2)3 Kp decreased

  5. Changing Temperature • Changing the temperature of a system will shift the position of an equilibrium and will change the value of Kc or Kp. 2NH3(g) ∆H = -92kJmol-1 exothermic N2(g) + 3H2(g) Decreasing temperature........... Favours exothermic forward reaction – trying give heat to system - equilibrium shifts to the right Increase in yield of NH3 This term increases Kp = (pNH3)2 (pN2)(H2)3 Kp increased

  6. Changing Temperature • Predict the change in Kp if the temperature is increased in the following reaction CO(g)+ 3H2(g) ∆H = +206kJmol-1 endothermic CH4(g) + H2O (g) Increasing temperature........... Favours forward reaction – trying remove heat from system - equilibrium shifts to the right Increase in yield of CO & H2 This term increases Kp = (pCO)(pH2)3 (pCH4)(pH2O)3 Kp increased

  7. Combustion engine problems N2(g) + O2(g) 2NO (g) Kc = 4 x 10-31 at 20oC (298K) but at combustion temperature in a car engine Kc = 8 x 10-9 at 800oC (1100K) Is this reaction likely to happen at room temperature? Explain your reasoning The temperature of the spark which ignites the fuel/air mixture is about 2500K. At this temperature, how does the value of Kc change? How will this affect the yield of NO? Is the reaction endothermic or exothermic? Explain your answer using the change in the value of Kc

  8. Combustion engine problems N2(g) + O2(g) 2NO (g) Kc = 4 x 10-31 at 20oC (298K) but at combustion temperature in a car engine Kc = 8 x 10-9 at 800oC (1100K) Is this reaction likely to happen at room temperature? Explain your reasoning Kc very small at room temperature therefore reaction unlikely. The temperature of the spark which ignites the fuel/air mixture is about 2500K. At this temperature, how does the value of Kc change? How will this affect the yield of NO? Kc = [NO]2 [N2][O2] Kc increases at higher temperatures Yield of NO increases Is the reaction endothermic or exothermic? Explain your answer using the change in the value of Kc

  9. Combustion engine problems N2(g) + O2(g) 2NO (g) Kc = 4 x 10-31 at 20oC (298K) but at combustion temperature in a car engine Kc = 8 x 10-9 at 800oC (1100K) Is the reaction endothermic or exothermic? Explain your answer using the change in the value of Kc Kc = [NO]2 [N2][O2] Endothermic – increased temperature, increased yield of NO. Increasing temperature favours an endothermic reaction – the system tries to remove the imposed heat

  10. Using a Catalyst • A catalyst speeds up the forward and backward reaction equally • The position of the equilibrium is not affected • However the system reaches equilibrium faster when a catalyst is used • Catalysts do not alter the value of Kc or Kp

  11. Factors that Affect Equilibrium • Changing concentration has no effect on Kc • Changing pressure has no effect on Kp • Catalysts have no effect on Kc • Changing temperature changes the position of the equilibrium and the value of Kc or Kp

More Related