Kinetics Flashcards

1
Q

How to identify the rate from a graph?

A

The gradient- Ea/RT

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2
Q

Maxwell-Boltzmann Distribution Curve properties

A
  • area under curve does not change because total number of particles remain constant
  • the most probable energy value is at the peak of the curve
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3
Q

Collision Theory-what must happen for a reaction to occur? (3things)

A
  1. Particles must collide
  2. They must collide with appropriate geometry
  3. Collide with sufficient energy
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4
Q

Activation energy

A

Minimum amount of energy required for a reaction to occur

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5
Q

How does Temperature affect the rate of reaction? Why?

A

Increase in temperature, increases rate of reaction

-more particles with sufficient energy to react thus more successful collisions

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6
Q

How does Concentration affect the rate of reaction?

A

Increasing concentration, increases rate of reaction

-increase number of particles in a given volume and so increases the chance of successful collision

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7
Q

How does Surface Area affect rate of reaction?

A

The smaller the particles the faster the reaction

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8
Q

How does catalysts affect the rate of reaction?

A

Presence of catalyst increases the rate of reaction
- provide an alternative pathway for the reaction with lower activation energy, and more reactants will possess lower Ea so rate increases

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9
Q

Rate Equation

A

Rate=k[A]x[B]y - A B= reactants!

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10
Q

What is the rate determining step?

A

The slowest step

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11
Q

What is Molecularity?

A

The number of particles reacting in the rate determining step of a reaction:
Unimolecular-1 species
Binolecular-2specieso

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12
Q

Arrhenius equation

A

K=Ae^(-Ea/RT)

A Arrhenius constant related to orientation of reactants

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13
Q

What are heterogeneous catalysts and how do they affect the rate reaction?

A

Catalyst in different phase than reactants- forms activated complex, weakening bonds and increasing collision-rate of reaction

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14
Q

What is an Activated complex?

A

An association of the reacting particles in which bonds are in the process of being broken and formed.
Either forms products or reverts to original reactants

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15
Q

Definition of Rate of Reaction?

A

The increase/decrease in the concentration of one of the products per unit time

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