equilibrium chemical reaction in which reactants are forming as fast as products yet the net...
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![Page 1: Equilibrium Chemical reaction in which reactants are forming as fast as products yet the net concentrations of each remains constant A + B C + D N 2](https://reader036.vdocuments.us/reader036/viewer/2022072006/56649cff5503460f949cff89/html5/thumbnails/1.jpg)
![Page 2: Equilibrium Chemical reaction in which reactants are forming as fast as products yet the net concentrations of each remains constant A + B C + D N 2](https://reader036.vdocuments.us/reader036/viewer/2022072006/56649cff5503460f949cff89/html5/thumbnails/2.jpg)
EquilibriumChemical reaction in which reactants are forming as fast as products yet the net
concentrations of each remains constant
A + B C + D
N2 + 3H2 2 NH3
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Equilibrium Constant K
aA + bB cC + dD
K = [C]c [D]d
[A]a [B]b
Products over reactants
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Equilibrium Constant K
K > 1000 mostly products
K < .001 mostly reactants
K = .001 to 1000 equilibrium condition
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Lechatlier’s Principle
If stress is applied to a system at equilibrium, the system will
adjust to relive the stress
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Lechatlier’s Principle
Possible stresses occur with Concentration, Volume and
Temperature
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Change in concentration
PCl3 + Cl2 PCl5
At equilibrium, the molar concentrations are constant
Add PCl5 the reaction will shift to form more PCl3 and Cl2
remove PCl5 the reaction will shift to form less PCl3 and Cl2Add PCl3 or Cl2 more PCl5 will form
Remove PCl3 and Cl2 more will form
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Change in volume
Reducing the volume or increasing the pressure causes the equilibrium to shift to the side of the
equation with the fewest moles
N2 g + 3H2 g 2NH3 g
4moles 2 moles
H2 g + Br2 g 2HBr g
2moles 2moles
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Temperature effects
Exothermic
Reactants products + Heat
H2 + O2 H2O + 700 Calories
Endothermic
Heat + Reactants products
CO2 + 2H2 + 90.7 Calories CH3OH
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Catalyst effect
A catalyst speeds up the rate at which equilibrium is achieved but does not change anything else – this occurs due to lowering
the activation energy
E
AB
EaEa