Chemistry- Equilibria and Redox Reactions (1.6)

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Dynamic Equilibrium
Concentration of reactants and products are constant. Forward and backwards reactions are going at the same rate. Must be closed system and at constant temperature, pressure and concentration.
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If reactants get used up...
Forward reaction slows.
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If products get used up...
Revers.e reaction slows
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If more products formed...
Reverse reaction speeds up.
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If more reactants formed...
Forward reaction speeds up.
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Le Chatlier's Principle
Change in conc, pressure or temp, position of equilibrium shifts to counteract the change. End up with different amounts of reactants and products.
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If position of equilibrium shifts to the left...
Reverse reaction is faster= more reactants.
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If position of equilibrium shifts to the right...
Forward reaction is faster= more products.
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If forward reaction is exothermic, and the temperature is increased...
Equilibrium will shift to cool the reaction down, so it will shift to the left (endothermic side), which decreases the product yield.
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If forward reaction is exothermic, and the temperature is decreased...
Equilibrium will shift to heat the reaction up, so it will shift to the right, so product yield increases. However, the rate of reaction is too low, so a compromise temperature must be found.
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If concentration is increased...
Equilribrium shifts to try to get rid of the extra reactant by making more product, or tries to get rid of teh extra product by making more reactants. Equilibrium shifts to the opposite side.
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If pressure is increased...
Equilibrium shifts to the side with the fewest molecules to reduce the pressure.
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Effect of catalyst on position of equilbrium:
No effect. Catalysts increase rate of reaction, not yield.
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Kc
Equilibrium constant. Ratio worked out from the concentrations of the products and reactants after equilibrium is reached. Only for that particular temperature.
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Kc Equation
[D]d [E]e / [A]a [B]b products/ reactants. Find moles at equilibrium and substitute in.
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Effect of Increasing Temperature on Kc
Increasing the temperature shifts equilibrium to the endothermic side. If the change means more product is formed, Kc will rise. If the change means less product is formed, then Kc will decrease.
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Effect of Increasing Concentration on Kc
The value of Kc is fixed at a given temperature, so if the concentration of one thing increases, then the concentrations of the rest will change (due to equilibrium shifting), to keep Kc the same.
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Effect of Adding a Catalyst to Kc
Catalysts increases the rate of both the forward and backwards reaction equally, so it has no effect on the position of equilbrium or Kc.
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OILRIG
Oxidation Is Loss, Reduction Is Gain (of electrons).
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Oxidising agent
Accepts electrons and is reduced.
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Reducing agent
Donates electrons and is oxidised.
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Oxidation State
Total number of electrons donated/accepted.
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What is the oxidation value for uncombined elements?
0
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What is the oxidation value of identical atoms bonded together?
0
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What is the oxidation value for a monatomic ion?
Same as it's charge.
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What is the oxidation value for a neutral compound?
0
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What is the oxidation value for combined oxygen?What about peroxides?
-2. Peroxides= -1.
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What is the oxidation value for uncombined hydrogen? What about hydrides? What about H2?
+1. Hydrides= -1. H2= 0.
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Step for writing out a full redox reaction:
1. Write out ionic half equations for oxidation and reduction. 2. Multiply by a factor to create the same number of electrons. 3. Cancel out anything found on both sides. 4. Rewrite full equation (perhaps put together products into a compound if n
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Other cards in this set

Card 2

Front

If reactants get used up...

Back

Forward reaction slows.

Card 3

Front

If products get used up...

Back

Preview of the front of card 3

Card 4

Front

If more products formed...

Back

Preview of the front of card 4

Card 5

Front

If more reactants formed...

Back

Preview of the front of card 5
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