Equilibrium

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  • Created by: Becca P
  • Created on: 01-04-13 13:35
What is equilibrium
rate of forward reaction equals rate of backward reaction
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concentrations at equilibrium
reactants and products are constant
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temperature increase favours
endothermic
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temperature decrease favours
exothermic
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increase in pressure favours
least moles of gas
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decrease in pressure favours
most moles of gas
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increase in concentration of reactants favours
products
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decrease in concentration of reactants favours
reactants
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catalyst effect on equilibrium position
no effect
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what is the equilibrium constant
ratio of conc of products divided by conc of reactants
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units of K
no units
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K<10-3
no reaction
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10-3<K<10+3
large quantities of products and reactants
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K>10+3
reaction is complete
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homogeneous equilibria
reactants and products are the same state
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heterogeneous equilibria
reactant and products are different states
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what affects the value of K
temperature
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increase in temp for endothermic what happens to K?
K increases
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increase in temp for exothermic what happens to K?
K decreases
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why must a vessel be closed at equilibrium
so no gases can escape and affect position of equilibria
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how to calculate K for reverse reaction
take inverse of K for forward reaction
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Other cards in this set

Card 2

Front

concentrations at equilibrium

Back

reactants and products are constant

Card 3

Front

temperature increase favours

Back

Preview of the front of card 3

Card 4

Front

temperature decrease favours

Back

Preview of the front of card 4

Card 5

Front

increase in pressure favours

Back

Preview of the front of card 5
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