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GCSE Chemistry > The Rate and Extent of Chemical Change > Flashcards

The Rate and Extent of Chemical Change Flashcards

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1
Q

How do we measure the rate of a reaction?

A
  • Measuring how fast the reactants are used up
    or
  • Measuring how fast the products are forms
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2
Q

Rate of Reaction Equation

A

Quantity of Reactants used up (g or cm3) /Time Taken (s)

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3
Q

Rate of Reaction Equation 2

A

Quantity of Products Formed (g or cm3) /Time Taken (s)

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4
Q

Mass of reactant on a graph

A
  • At first decreases rapidly
  • Slows as reaction progresses (reactant gets used up less quickly)
  • Mass of reactant is 0
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5
Q

Volume of product on a graph

A
  • Starts at 0 (no products yet)
  • Quickly increases as product is formed
  • Graph becomes less steep
  • Eventually plateau’s (levels off) when a reactant is used up
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6
Q

What affects the rate of a reaction?

A
  • Temperature
  • Surface Area
  • Absence/Presence of catalysts
  • Concentration/Pressure
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7
Q

Collision Theory

A

For particles to react, they have to collide with each other with a sufficient amount of energy

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8
Q

What factors affect collision theory?

A
  • Amount of energy the particles have (more energy means more energy transfer during collisions)
  • Frequency of collisions (more frequent collisions mean more successful ones)
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9
Q

How does temperature increase rate of reaction?

A
  • Temp. increase means particles gain more energy
  • Particles move faster
  • More frequent collisions
  • Collide with more energy
  • More likely to exceed activation energy
  • More successful collisions
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10
Q

How does concentration/pressure increase rate of reaction

A
  • Increase in concentration/pressure means increase in particles (per unit of volume)
  • More frequent collisions
  • More successful collisions
  • Increase in reaction rate
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11
Q

How does surface area increase rate of reaction?

A
  • Increase in surface area means higher SA:V ratio
  • More frequent collisions
  • Higher rate of successful collisions
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12
Q

Catalyst

A

Substances that speed up rate of reaction without being used up (aren’t included in the reaction equation)

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13
Q

How do catalysts increase rate of reaction?

A
  • Lower activation energy by providing alternative reaction pathways
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14
Q

What is a Reversible Reaction?

A

A chemical reaction that can happen in both directions

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15
Q

What is Equilibrium?

A

When the concentrations of the forward and backward reactions of a reversible reaction remain constant

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16
Q

Where does the equilibrium lie when there are more products?

A

To the right of the equation

17
Q

Where does the equilibrium lie when there are more reactants?

A

To the left of the equation

18
Q

What conditions impact the position of equilibrium?

A

-Temperature
-Pressure
-Concentration

19
Q

When can equilibrium be reached?

A

When the reversible reaction is done in a closed system

20
Q

What is Le Chatelier’s Principle?

A

When changing the conditions of a reversible reaction, the position of equilibrium will change to counteract the change

21
Q

What happens when the temperature of a reversible reaction is decreased?

A

The position of equilibrium moves the side of the reaction that is exothermic. Exothermic reactions create temperature increase and that counteracts the decrease

22
Q

What happens when the temperature of a reversible reaction is increased

A

The position of equilibrium moves the side of the reaction that is endothermic. Endothermic reactions create temperature decrease and that counteracts the increase

23
Q

What happens when the pressure of a reversible reaction is increased?

A

The position of equilibrium moves to the side of the equation with the least molecules

24
Q

What happens when the pressure of a reversible reaction is decreased?

A

The position of equilibrium moves to the side of the equation with the most particles

25
Q

What happens when the concentration of a reversible reaction is increased?

A

The position of the equilibrium moves to the other side of the equation and produces more product/reactant (depends on what side the equilibrium was initially on)

26
Q

What happens when the concentration of a reversible reaction is decreased?

A

The position of the equilibrium moves to the other side of the equation and produces less product/reactant (depends on what side the equilibrium was initially on)

27
Q

Pressure only impact substances in what state?

A

Gaseous

GCSE Chemistry (7 decks)

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