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15 Cards in this Set
- Front
- Back
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Activation energy
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The minimum amount of energy required for the reaction to take place.
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Effects of increase in temperature
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The particles have more energy, increasing the probability of successful collisions. More collisions = higher rate.
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Effects of increase in concentration
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More particles in the given volume. More particles = more successful collisions.
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Effects of adding a catalyst
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Lowers activation energy so more particles have the required energy to take part in the reaction, increasing the probability of successful collisions.
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Arrhenius equation
-Ea/RT K= Ae |
K= rate constant
Ae= factor linked to orientation and frequency of collisions Ea= activation energy R= gas constant (8.13 Jk-1 mole-1) T= temperature (K) |
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0 order
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Rate doesn't change
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1st order
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Proportionate: double the concentration, rate doubles
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2nd order
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Double the concentration, rate quadruples
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Half life
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The time taken for the concentration of the reactant to fall to half of its initial value.
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Rate expression
Rate = K (A)^x (B)^y |
K= rate constant
(A)= concentration of A (B)= concentration of B x +y= overall order |
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Catalysed
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With a catalyst.
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Uncatalysed
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Without a catalyst.
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Rate of reaction
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Speed of which the reactants are used up or new products are formed.
Units: conc/ time, eg mol dm/ s |
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Rate determining step
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The slowest step of a reaction. This determines the rate of the entire reaction.
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Rate constant
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The constant of proportionality in the rate expression. Unit is: (mol dm-3)1 – overall order s-1.
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