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Reaction Kinetics (Defintions (Order of reaction (The power to which the…
Reaction Kinetics
Defintions
Rate equation
An equation showing the relationship between the concentrations of the reactants that affect the rate of equation and the rate constant.
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Order of reaction
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If the concentration does not affect the rate, the reaction is zero order
If the concentration is directly proportional to the rate, the reaction is first order.
If the rate is directly proportional to the square of the reactant concentration, the reaction is second order.
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Half-life of a reaction
The amount of time taken for the amount (or concentration) of the limiting reactant in a reaction to decrease by half of its value.
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Activation energy
The minimum energy that colliding particles must posses for a successful collision that results in a reaction to take place.
Enzymatic activity
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They speed up a reaction without being used up and provides an alternative reaction pathway with a lower activation energy
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Collision frequency
Concentration changes
With the same volume, increasing the concentration will increase the rate of reaction
This is due to the fact that the random motion of the particles in the solution will result in a more frequent collisions between the reacting particles
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Temperature changes
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The increased energy will result in the particles to move around more quickly (as they have more kinetic energy), causing the increasing of frequency of collisions.
Pressure changes
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As we increase the pressure of reacting gases, we will decrease the volume; thus, the same amount of molecules will be contained in a smaller place so more collisions will happen in a given time
Boltzmann Distribution
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Effect of catalyst
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Catalyst provides a lower activation energy so a greater proportion of molecules in the reaction mixture have sufficient energy to react.
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