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Chemistry > Chapter 9 > Flashcards

Chapter 9 Flashcards

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1
Q

What are particles in liquids and gases always doing?

A

They are always moving and colliding with each other

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2
Q

What are the 2 conditions for a reaction to take place?

A
  • They collide in the right direction. They need to be facing each other
  • They must collide with enough energy
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3
Q

What is the collision theory?

A

The conditions for the reaction to occur.

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4
Q

What is the activation energy?

A

The minimum amount of kinetic energy particles need to react

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5
Q

Why do the particles need the activation energy for the reaction to start?

A

So the bonds can break

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6
Q

How do you give particles energy?

A

By heating them

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7
Q

What reaction will happen easier, reactions with low activation energies or reactions with high activation energies?

A

Reactions with low activation energies, as less energy is required

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8
Q

Do molecules all have the same amount of energy?

A

No

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9
Q

What does a Maxwell-Boltzmann Distribution show you

A

The amount of molecules which have the required activation energy

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10
Q

Why does a Maxwell-Boltzmann distribution start at (0,0)?

A

Because no molecules have 0 energy

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11
Q

What energy do molecules have to have in order to react?

A

> the activation energy

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12
Q

What does increasing the temperature do?

A

It increases the reaction rate

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13
Q

If you increase the temperature, what will the particles have more of on average?

A

More kinetic energy so will move faster

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14
Q

What will differ with a Maxwell-Boltzmann distribution when you increase the temperature?

A

More molecules will have the required activation energy

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15
Q

If molecules are flying about faster, what will they do more often?

A

They’ll collide more often

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16
Q

What does increasing the concentration do to the reaction rate?

A

It increases the reaction rate

17
Q

Why does increasing the concentration increase the reaction rate?

A

More particles in a given volume, so particles will collide more frequently

18
Q

What does increasing the pressure do to the reaction rate?

A

It increases the reaction rate

19
Q

Why does increasing the pressure increase the reaction rate?

A

More particles in a given volume of gas, so more collisions

20
Q

What does a catalyst do to the reaction rate?

A

It increases the reaction rate

21
Q

What do catalysts do?

A

They lower the activation energy, by providing a different way for bonds to be broken and remade

22
Q

What is the reaction rate?

A

The change in the amount of reactant or product per unit time

23
Q

Why would you use a catalyst?

A

To increase the reaction rate

24
Q

Do catalysts get used up in the reaction?

A

No

25
Q

What is a heterogeneous catalyst?

A

One that is in a different phase from the reactants

26
Q

In a reaction containing a heterogeneous catalyst, where does the reaction occur?

A

On the surface of the catalyst

27
Q

What does increasing the surface area of the heterogeneous catalyst do?

A

It increases the rate of reaction, as there are more molecules that can react at the same time.

28
Q

How does a heterogeneous catalyst work?

A

By lowering the activation energy of the reaction

29
Q

What is adsorption?

A

When reactant molecules arrive at the surface and bond with the solid catalyst

30
Q

What happens to the bonds between the reactant’s atoms during adsorption?

A

They are weakened and break up

31
Q

How are radicals formed during adsorption?

A

The bonds between the reactant’s atoms are weakened and break up, which form atoms or molecules with unpaired electrons.

32
Q

What do the radicals do once formed by adsorption?

A

They get together and form new molecules

33
Q

What is desorption?

A

When the new molecules are detached from the catalyst

Chemistry (25 decks)

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