3.2 Controlling the rate Flashcards

1
Q

collision theory

A

Reaction rates must be controlled in industrial processes. If the rate is too low then the process will not be economically viable, if it is too high there will be a risk of explosion.

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2
Q

what effects on reaction rates can be explained with the collision theory?

A

 concentration
 pressure
 surface area (particle size)
 temperature
 collision geometry

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3
Q

enthalpy change

A

The enthalpy change is the energy difference between the products and the reactants. The enthalpy change has a negative value for exothermic reactions or a positive value for endothermic reactions.

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4
Q

activation energy

A

The activation energy is the minimum energy required by colliding particles to form an activated complex and can be calculated from potential energy diagrams

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5
Q

activated complex

A

The activated complex is an unstable arrangement of atoms formed at the maximum of the potential energy barrier, during a reaction.

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6
Q

effect of catalyst on reaction pathway

A

A catalyst provides an alternative reaction pathway with a lower activation energy.

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7
Q

Temperature

A

Temperature is a measure of the average kinetic energy of the particles in a substance.

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8
Q

Activation energy

A

The minimum kinetic energy required by colliding particles before a reaction may occur

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9
Q

How can you explain the effects of temperature and adding a catalyst?

A

In terms of a change in the number of particles with energy greater than the activation energy

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