Chemistry (Factors affecting Rate of Reaction) Flashcards

1
Q

What does the reaction rate depend on?

A

Nature of the reactants.

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2
Q

Increasing the concentration of reactants…

A

Increases rate of reaction.

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3
Q

Increasing the pressure and decreasing volume is equivalent to…, and therefore…

A

increasing the concentration, and therefore increases the rate of reaction.

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4
Q

Closer particles…

A

Causes more frequent collisions

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5
Q

More frequent collisions means…

A

the proportion of particles can react together.

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6
Q

Increasing the surface area…

A

Increases the number of reactant particles available for collisions.

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7
Q

Increasing the surface area increases… which therefore increases..

A

Increases collisions, therefore increasing rate of reaction.

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8
Q

Creating movement in a fluid is called?

A

Agitation

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9
Q

Agitation decreases/increases collisions?

A

(Increases) Particles are more exposed for collisions but they are given more kinetic energy.

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10
Q

A greater proportion of particles that have been agitated are given more… therefore have energy…

A

Given more kinetic energy and therefore have greater energy than the activation energy.

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11
Q

An increase in temperature…

A

Increases the rate of a chemical reaction.

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12
Q

When a substance gets hot its particles… and have more…

A

Particles vibrate and have more kinetic energy.

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13
Q

Increase in KE causes particles to

A

Move faster and have more frequent collisions.

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14
Q

A greater proportion of particles that have been increased in temperature are given more… therefore have energy…

A

Given more kinetic energy and therefore have greater energy than the activation energy.

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15
Q

What is a catalyst?

A

Something that can speed up or slow down a chemical reaction.

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16
Q

A positive catalyst …. reaction rate

A

Increases

17
Q

A negative catalyst … reaction rate

A

Decreases

18
Q

Catalysts increase reaction rate by …. that has a …..

A

providing an alternate reaction pathway that has a lower activation energy.

19
Q

A greater proportion of particles that have been catalysed are given more… therefore have energy…

A

Have a more sufficient energy and therefore have enough energy to overcome the activation energy.

20
Q

Describe the effect that catalysts have on the hill part of an energy profile diagram.

A

The hill of the energy profile diagram moves down if the reaction is catalysed. This provides an alternate reaction pathway which is why the activation energy is lower.

21
Q

Explain, using collision theory, why an increase in temperature can result in an increase in rate of reaction?

A
  • Energy increase means the energy becomes greater than the activation energy.
  • Kinetic energy in particles increase
  • Movement and vibration increase causes more collisions
  • Increase in collisions increases the rate of reaction
22
Q

Explain, using collision theory, why diluting a solution can result in a reduction in rate of reaction?

A
  • Concentration decreases
  • Increase difficulty in particles to collide, meaning less collisions
  • Further apart, less collisions means less reactant particles
  • Decreases in particles colliding with less collisions in the correct orientation.
23
Q

Explain, using collision theory, why grinding a soil sample to a small particle size can result in an increase in rate of reaction?

A
  • Increase in surface area
  • Increase in the reactant particles
  • Increase in likelihood of collisions with correct orientation.
24
Q

Explain, using collision theory, why the introduction of an inert gas (such as nitrogen) into a closed (sealed) chemical system can result in an increase in rate of reaction?

A
  • Introduction of a gas in a closed system increases pressure
  • Increase in pressure decreases volume
  • Decrease in volume allows a higher chance of collisions with the reactant particles.
    Increase in collisions increases the reaction rate.
25
Q

Explain, using collision theory, why the addition of a catalyst into a reaction mixture can result in an increase in rate of reaction?

A
  • Catalysts provide an alternate reaction pathway giving an alternate lower required activation energy.
  • This increases the proportion of particles that have sufficient energy to react.
  • Sufficient energy means that the particles have greater energy than the activation energy
  • This will increase the likelihood of collisions increasing the rate of reaction.