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Chem Eq Lec2v3
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Chem Eq Lec2v3

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  • 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?

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