6. Chemical Kinetics Flashcards

1
Q

What is rate of reaction?

A

The change in concentration of a reactant or product over time.

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2
Q

What are the units of rate of reaction?

A

moldm-3s-1

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3
Q

What are the assumptions of kinetic molecular theory?

A
  • Particles are in constant motion.
  • All collisions are elastic
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4
Q

What must happen for a reaction to occur?

A
  • The particles must collide with each other with sufficient energy (Ea)
  • The particles must collide in the correct orientation
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5
Q

What is activation energy?

A

The minimum energy needed for a reaction to occur on colliding of particles.

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6
Q

What does a Maxwell-Boltzmann curve show?

A

Shows the energy distribution in a sample of molecules.

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7
Q

What is the area under a Maxwell-Boltzmann curve?

A

The total number of particles.

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8
Q

What factors affect the rate of reaction?

A
  • Surface area
  • Temperature
  • Concentration
  • Pressure/ volume
  • Catalysts
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9
Q

Why are catalysts not included in chemical equations?

A

They are not used up.

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10
Q

How do catalysts work?

A

They lower the activation energy of a reaction by providing an alternate reaction pathway with a lower activation energy.

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11
Q

Explain how an increase in concentration/pressure affects the rate of reaction.

A
  • Number of particles per given volume increases
  • Increased number of frequent (successful collisions)
  • Rate increases
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12
Q

Explain how an increase in surface area affects the rate of reaction.

A
  • Exposes more reactant particles
  • Increased number of collisions and successful collisions per second
  • Increased rate of reaction
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13
Q

Explain the effect of an increase in temperature on the rate of reaction

A
  • Increased energy, so KE of particles increases
  • A greater proportion of the particles have the required activation energy
  • More collisions per second
  • Increased number of collisions result in a reaction
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14
Q

What are the two major economic advantages of the use of catalysts in industry?

A
  • They increase the rate of a chemical reaction meaning that more of the desired product can be made in a given time period
  • Reactions can take place at lower temperatures resulting in a decrease in the energy costs to the manufacturer
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15
Q

What is a heterogeneous catalyst?

A

A catalyst that is in a different phase to the reactants

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16
Q

What are 3 ways of monitoring concentration changes in a reaction?

A
  • Mass (loss of mass as gas released)
  • Volume (of gas produced)
  • Colour ( production of solid and cross)