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Chemical Equilibrium Presentation Part 2 c!e-γ˚T 2010
KP and KC equation Derive  Kp= Kc(RT)n n = (moles of gaseous product)  		− (moles of gaseous reactant) If n= 0        then KC= KP n> 0        then KC< KP n< 0        then KC> KP H2(g) + Br2(g) HBr(g) N2O5(g)  NO2 + O2(g) CaCO3 (s) CaO (s) + CO2(g) AgCl (s)  Ag+ (aq) + Cl- (aq) (NH4)2Se (s)  NH3 (g) + H2Se (g)
Solving for KC and KP Carbonyl chloride (COCl2), also known as phosgene was used in World War I as a poisonous gas.  The equilibrium concentrations for the reaction between carbon monoxide and chlorine gas to form phosgene at 74oC are [CO] = 1.2x10-2 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate KC and KP.  (220, 7.6) Consider the following equilibrium process at 700oC: 2H2 (g) + S2 (g)  2H2S (g).  Analysis shows that there are 2.50 moles of H2, 1.35x10-5moles S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate KC for the reaction.  (1.08 x107 ) The equilibrium constant KP for the reaction        2NO2 (g)  2NO (g) +O2 (g) is 158 at 1000 K.  Calculate PO2 if      PNO2 = 0.400 atm and PNO = 0.270 atm. (347 atm)
Manipulating equilibrium constants Reversing a chemical equation 2NO2 (g)  N2O4 (g)	KC = 4.63 X 10-3 N2O4 (g)  2NO2 (g) 	K’C = ?
Manipulating equilibrium constants Multiplying or dividing coefficients by a constant 2NO2 (g)  N2O4 (g)	KC = 4.63 X 10-3 6NO2 (g)  3 N2O4 (g)	K”C = ? NO2 (g)  ½ N2O4 (g)	K’”C = ?
Manipulating equilibrium constants Adding chemical reactions
Example 2N2 (g) + O2 (g) 2N2O (g)	KC = 7.29 X 10-36 N2 (g) + O2 (g) 2NO (g)	KC = 4.70 X 10-31 N2O (g) + ½ O2  (g) 2NO (g)	KC = ?
Predicting direction of a reaction to achieve equilibrium K   >  Q,  K   -- >  Q K  <  Q, K   < --   Q K   =  Q, K  < = >  Q
Example The equilibrium constant for the formation of nitrosyl chloride from nitric oxide and molecular chlorine:  2NO (g) + Cl2 (g)  2 NOCl (g)  is 6.5 x 104 at 35 oC.  In a certain experiment, 0.02 mole of NO, 0.0083 mole of Cl2 and 6.8 mole NOCl are mixed in 2.0 L flask, in which direction will the system proceed to reach equilibrium?

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Chem Eq Lec2v3

  • 1. Chemical Equilibrium Presentation Part 2 c!e-γ˚T 2010
  • 2. KP and KC equation Derive Kp= Kc(RT)n n = (moles of gaseous product) − (moles of gaseous reactant) If n= 0 then KC= KP n> 0 then KC< KP n< 0 then KC> KP H2(g) + Br2(g) HBr(g) N2O5(g)  NO2 + O2(g) CaCO3 (s) CaO (s) + CO2(g) AgCl (s)  Ag+ (aq) + Cl- (aq) (NH4)2Se (s)  NH3 (g) + H2Se (g)
  • 3. Solving for KC and KP Carbonyl chloride (COCl2), also known as phosgene was used in World War I as a poisonous gas. The equilibrium concentrations for the reaction between carbon monoxide and chlorine gas to form phosgene at 74oC are [CO] = 1.2x10-2 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate KC and KP. (220, 7.6) Consider the following equilibrium process at 700oC: 2H2 (g) + S2 (g)  2H2S (g). Analysis shows that there are 2.50 moles of H2, 1.35x10-5moles S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate KC for the reaction. (1.08 x107 ) The equilibrium constant KP for the reaction 2NO2 (g)  2NO (g) +O2 (g) is 158 at 1000 K. Calculate PO2 if PNO2 = 0.400 atm and PNO = 0.270 atm. (347 atm)
  • 4. Manipulating equilibrium constants Reversing a chemical equation 2NO2 (g)  N2O4 (g) KC = 4.63 X 10-3 N2O4 (g)  2NO2 (g) K’C = ?
  • 5. Manipulating equilibrium constants Multiplying or dividing coefficients by a constant 2NO2 (g)  N2O4 (g) KC = 4.63 X 10-3 6NO2 (g)  3 N2O4 (g) K”C = ? NO2 (g)  ½ N2O4 (g) K’”C = ?
  • 6. Manipulating equilibrium constants Adding chemical reactions
  • 7. Example 2N2 (g) + O2 (g) 2N2O (g) KC = 7.29 X 10-36 N2 (g) + O2 (g) 2NO (g) KC = 4.70 X 10-31 N2O (g) + ½ O2 (g) 2NO (g) KC = ?
  • 8. Predicting direction of a reaction to achieve equilibrium K > Q, K -- > Q K < Q, K < -- Q K = Q, K < = > Q
  • 9. Example The equilibrium constant for the formation of nitrosyl chloride from nitric oxide and molecular chlorine: 2NO (g) + Cl2 (g)  2 NOCl (g) is 6.5 x 104 at 35 oC. In a certain experiment, 0.02 mole of NO, 0.0083 mole of Cl2 and 6.8 mole NOCl are mixed in 2.0 L flask, in which direction will the system proceed to reach equilibrium?