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Slide 1

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EQUILIBRIA…read more

Slide 2

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Equilibrium Basics
· When a reversible reaction can form the products from the
reactants and vice versa
· Dynamic Equilibrium: a reversible reaction where the
forward and backwards reactions are equal and there
concentrations are constant
· Heterogeneous- Species are in different phases
· Homogeneous- All species are in the same phase…read more

Slide 3

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The Equilibrium Constant, Kc
· As long as temperature is constant Kc can be calculated
· The units are different for each reaction e.g.
· N2 + 3H2 2NH3
· Kc =
· Units: [(mol dm-3)2]/[(mol dm-3) x (mol dm-3)3] = mol-2 dm6…read more

Slide 4

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Effects of Changing Conditions:
Forward Temperature Equilibrium Yield of Rate of Kc
Reaction Position Product Attainment
Exothermic Increase Shifts left Decrease Increase Decrease
Exothermic Decrease Shifts right Increase Decrease Increase
Endothermic Increase Shifts right Increase Increase Increase
Endothermic Decrease Shifts left Decrease Decrease Decrease…read more

Slide 5

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Effects of Changing Conditions:
Larger Mole Pressure Kc * Equilibrium Yield of
Position Product
Reactant Increase - Shifts right Increase
Reactant Decrease - Shifts left Decrease
Product Increase - Shifts left Decrease
Product Decrease - Shifts right Increase
*Kc is not affected by pressure, concentration or a catalyst…read more

Slide 6

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The Position of Equilibrium
· If Kc is greater than 1, products predominate over
reactants so equilibrium is to the right
· If Kc is less than 1, reactants predominate over products
so equilibrium is to the left
· Reactions where Kc is greater than 1010 are going to
completion…read more

Slide 7

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