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Chemistry > 4.1 Rates of Reaction > Flashcards

4.1 Rates of Reaction Flashcards

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1
Q

How can chemical reactions only happen?

A

If reactant particles collide with enough energy

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2
Q

What is Activation Energy?

A

The amount of energy needed to make particles react

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3
Q

What is Collision Frequency?

A

How often the particles collide with each other

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4
Q

What is Percentage Success?

A

What percentage of collisions have enough energy

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5
Q

What 4 factors effect the rate of reaction?

A

Collision Frequency:
- Solid surface area
- Solution concentration
Percentage Success:
- Temperature
- Catalysts

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6
Q

Why does a higher surface area increase rate of collisions?

A
  • More of solid is exposed to the other particles
  • So collisions frequency is higher
  • Therefore more successful collisions per unit time
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7
Q

Why does a higher solution concentration increase rate of collisions?

A
  • More particles per unit volume
  • So collision frequency is higher
  • Therefore more successful collisions per unit time
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8
Q

Why does a higher temperature increase the rate of collisions?

A
  • Particles have more kenetic energy
  • So percentage of collisions with enough energy is higher
  • Therefore more successful collisions per unit time
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9
Q

Why do catalysts increase the rate of collisions?

A
  • Provide an alternate route with lower activation energy
  • So Percentage of collisions with enough energy is higher
  • Therefore more successful collisions per unit time
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10
Q

How it increase surface area of a solid?

A

Cutting up or grinding

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11
Q

What experiment demonstrates the effect of surface area on rate?

A

Marble chip experiment

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12
Q

What is used in the marble chip experiment?

A

Calcium carbonate chips and hydrochloric acid

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13
Q

What are the control variables in the marble chip experiment?

A

-Mass of calcium carbonate chips
- Volume and concentration of HCl
- Temeprature

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14
Q

Why in solutions and gases, increasing the concentration/pressure increases rate?

A
  • There are more particles per unit volume
  • So the collision frequency is higher
  • More successful collisions per unit time
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15
Q

How can you easily increase pressure?

A

Make reaction vessel smaller

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16
Q

What experiment demonstrates the affect of concentration on rate?

A

Disappearing cross experiment

17
Q

What are the control variables in the disappearing cross experiment?

A
  • Total volume of solution
  • Concentration of HCl
  • Temperature
18
Q

How is rate calculated?

A

Rate = 1/time taken

19
Q

What does a straight line through the origin show on a concentration-rate graph?

A

Rate is proportional to concentration…
Double concentration = double rate

20
Q

What experiment demonstrates the effect of temperature on rate?

A

Magnesium and acid experiment

21
Q

What are the control variables in the magnesium and acid experiment?

A
  • Mass and surface area of magnesium
  • Volume and concentration of HCl
22
Q

Is rate proportional to temperature in the magnesium and acid experiment?

A

No
- The graph does not show a straight line
- The line does not go through the origin (as the rate isn’t zero at 0°C)

23
Q

What are catalysts?

A
  • Increase rate
    Remain chemically unchanged
24
Q

What experiment demonstrates the effect of different catalysts on rate?

A

Hydrogen peroxide experiment

25
Q

What are control variables in the hydrogen peroxide experiment?

A
  • Volume and concentration of H2O2
  • Temperature
  • Mass and surface area of catalyst
26
Q

How does a catalyst-rate graph show the effectiveness of a catalyst?

A

More effective, the steeper the line

Chemistry (18 decks)

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