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Chemical Equilibrium<br />Presentation Part 2<br />c!e-γ˚T 2010<br />
KP and KC equation<br />Derive  Kp= Kc(RT)n<br />n = (moles of gaseous product) <br />		− (moles of gaseous reactant)<br...
Solving for KC and KP<br />Carbonyl chloride (COCl2), also known as phosgene was used in World War I as a poisonous gas.  ...
Manipulating equilibrium constants<br />Reversing a chemical equation<br />2NO2 (g)  N2O4 (g)	KC = 4.63 X 10-3<br />N2O4 ...
Manipulating equilibrium constants<br />Multiplying or dividing coefficients by a constant<br />2NO2 (g)  N2O4 (g)	KC = 4...
Manipulating equilibrium constants<br />Adding chemical reactions<br />
Example<br />2N2 (g) + O2 (g) 2N2O (g)	KC = 7.29 X 10-36<br />N2 (g) + O2 (g) 2NO (g)	KC = 4.70 X 10-31<br />N2O (g) + ½...
Predicting direction of a reaction to achieve equilibrium<br />K   &gt;  Q,  K   -- &gt;  Q<br />K  &lt;  Q, K   &lt; --  ...
Example<br />The equilibrium constant for the formation of nitrosyl chloride from nitric oxide and molecular chlorine:<br ...
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Chem Eq Lec2v3

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Chem Eq Lec2v3

  1. 1. Chemical Equilibrium<br />Presentation Part 2<br />c!e-γ˚T 2010<br />
  2. 2. KP and KC equation<br />Derive Kp= Kc(RT)n<br />n = (moles of gaseous product) <br /> − (moles of gaseous reactant)<br />If n= 0 then KC= KP<br />n&gt; 0 then KC&lt; KP<br />n&lt; 0 then KC&gt; KP<br />H2(g) + Br2(g) HBr(g)<br />N2O5(g)  NO2 + O2(g)<br />CaCO3 (s) CaO (s) + CO2(g)<br />AgCl (s)  Ag+ (aq) + Cl- (aq)<br />(NH4)2Se (s)  NH3 (g) + H2Se (g)<br />
  3. 3. Solving for KC and KP<br />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)<br />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 )<br />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)<br />
  4. 4. Manipulating equilibrium constants<br />Reversing a chemical equation<br />2NO2 (g)  N2O4 (g) KC = 4.63 X 10-3<br />N2O4 (g)  2NO2 (g) K’C = ?<br />
  5. 5. Manipulating equilibrium constants<br />Multiplying or dividing coefficients by a constant<br />2NO2 (g)  N2O4 (g) KC = 4.63 X 10-3<br />6NO2 (g)  3 N2O4 (g) K”C = ?<br />NO2 (g)  ½ N2O4 (g) K’”C = ?<br />
  6. 6. Manipulating equilibrium constants<br />Adding chemical reactions<br />
  7. 7. Example<br />2N2 (g) + O2 (g) 2N2O (g) KC = 7.29 X 10-36<br />N2 (g) + O2 (g) 2NO (g) KC = 4.70 X 10-31<br />N2O (g) + ½ O2 (g) 2NO (g) KC = ?<br />
  8. 8. Predicting direction of a reaction to achieve equilibrium<br />K &gt; Q, K -- &gt; Q<br />K &lt; Q, K &lt; -- Q<br />K = Q, K &lt; = &gt; Q<br />
  9. 9. Example<br />The equilibrium constant for the formation of nitrosyl chloride from nitric oxide and molecular chlorine:<br /> 2NO (g) + Cl2 (g)  2 NOCl (g)<br /> 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?<br />

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