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Chemistry > Kinetics > Flashcards

Kinetics Flashcards

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1
Q

Collision frequency

A

? The number of collisions between particles per second.

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2
Q

Rate of reaction

A

? The change in concentration of a substance per unit time.

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3
Q

Activation energy

A

? The minimum energy required for the reaction to occur.

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4
Q

Catalyst

A

? provides an alternative reaction pathway with lower activation energy but remains chemically unchanged.

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5
Q

Heterogeneous Catalyst

A

? Catalyst that is in a different phase as the reactants

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6
Q

Homogeneous Catalyst

A

? Catalyst that is in the same phase as the reactants

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7
Q

What are the conditions for particles to react.

A
  • Energy higher than the activation energy

- The correct orientation

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8
Q

Describe the maxwell boltzman distribution curve.

A

Image that looks like a hill
x axis - energy
y axis - Number of particles with E.

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9
Q

Factors affecting rate of reaction

A
  • Concentration
  • Temperature
  • Pressure
  • Catalyst
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10
Q

How does increasing the temperature affect the maxwell boltzman curve.

A

Flattens and shifts to the right.

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11
Q

Can you explain the qualitative effect of temperature changes on the rate of reaction?

A

Higher temperature, higher frequency of collisions, which increases the number of successful collisions. Higher temperature, more particles have energy higher than the activation energy, thus the rate of reaction increases.

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12
Q

Can you explain the qualitative effect of changes in concentration on the ROR.

A

There are more particles per unit volume, thus the frequency of collisions increases, which increases the number of successful collisions, increasing the rate of reaction.

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13
Q

Can you describe the qualitative effect of a change in the pressure on ROR

A

Higher pressure, higher frequency of collisions, higher number of successful collisions, higher ROR

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14
Q

Can you describe a maxwell Boltzman reaction to explain the increased rate of reaction?

A

The line of Ea shifts to the left, thus more particles have an energy greater than the activation energy.

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15
Q

What is the purpose of a catalytic converter?

A

Purpose - to remove pollutant gases formed in internal combustion of the engine.
Construction - finely divided powders of alloys of platinum,rhodium and palladium spread onto a ceramic honeycomb structure

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16
Q

How does a catalyst work.

A

The reactants adsorb onto the surface. Adsorption weakens the bonds within the reactants. The catalyst provides them a surface for reaction, holding them in just the correct orientation. The product desorb from the surface.

17
Q

Poisoning

A

? Occurs when a species binds (almost) irreversibly to the catalyst surface. (lead)

This blocks the active site and prevents the reactants from adsorbing, thus decreasing the rate of reaction. It is expensive to recondition a catalyst

18
Q

Rate Equations/Law

A

? Shows the relationship between the species and their concentration on the rate of the reaction. Note that not all the reactants feature in the rate equation.

19
Q

Rate constant (k)

A

? A constant that shows the relationship between the rate and the varying molar species concentration.
? Proportionality constant that indicates the relationship between the molar concentration of reactants and the rate of a chemical reaction.
* Not affected by stoichiometry, determined by experimental data

Independent of concentration and time. It is a constant at fixed temperature.

20
Q

What is not included in the rate equation

A
  • catalyst
  • intermediate
  • products
21
Q

Rate order

A

? The mathematical relationship between the concentration of a species and the rate of the reaction.
Overall rate order: sum total of the rate order of each component determining the rate equation.

22
Q

What is the rate equation

A

Rate = k [A]^m[B]^n

23
Q

Can you describe a 0,1,2 order graph.

A

0 order - horizontal straight line
1 order - linear line
2 order - curve (quadratic)

24
Q

What effects does the order have on the ROR

A

0 - no effect
1 - directly proportional to A
2 - directly proportional to A^2

25
Q

Rate determining step

A

? The slowest step of a chemical reaction determines the rate at which the overall reaction proceeds. Only reagents in or before the rate-determining step will be included in the rate equation.
* Only reactants can be in the rate equation, not intermediates

26
Q

Intermediate

A

? A substance formed as a product from one step of a reaction, that reacts further to form a product of the overall reaction.

27
Q

What is the Arrhenius equation

A

k = Ae^(-Ea/RT)

Ea needs to be inJ/mol

28
Q

Half life of a reaction

A

? Time taken for the concentration of a substance to fall to half its original value.

Chemistry (11 decks)

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