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Chemistry > C6 > Flashcards

C6 Flashcards

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1
Q

what is gas pressure?
(prior knowledge)

A

the force exerted when gas particles collide with the surface of their container

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2
Q

what must happen before the reaction will start?

A

the particles must collide with enough activation energy

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3
Q

what does rate a measurement always have to include?

A

a measurement of mass or volume (of a substance) and a measurement of time

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4
Q

what is the definition of rate of reaction?

A

when the mass or volume of reactants change into products over a period of time

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5
Q

what is the definition of concentration?

A

the mass of solute within a certain volume (of solvent)

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6
Q

why is activation energy required?

A

to break bonds in the reactants

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7
Q

when is a reaction fastest?

A

at the start

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8
Q

why does a reaction slow down as it progresses?

A

there are little reactants left –> so there are less frequent successful collisions

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9
Q

dk the question to this answer

A

high concentration of reactant particles so more successful frequent collisions

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10
Q

what happens to the rate of reaction when the concentration is increased? why?

A

also increase because there are more reactant particles per unit volume

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11
Q

what happens to the mass or volume of a product if the concentration is increased?

A

stays the same

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12
Q

define random error.

A

variability between different measurements

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13
Q

what happens to the rate of reaction when you increase concentration? why?

A

increases - because there are more reactant particles in the same volume –> so there are more successful frequent collisions –> so the rate increases

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14
Q

when does a reaction stop?

A

when 1 or more reactants has been used up (limiting reactant)

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15
Q

what graph do we use to present continuous data?

A

line graph

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16
Q

state 2 ways to increase the rate of reaction?

A
  1. increase the temperature
  2. increase concentration of reactants
17
Q

why is carbon dioxide a gas at room temperature?

A

because it is a simple covalent molecule with weak intermolecular forces between the molecules so little energy is needed to break the forces

18
Q

define intervals

A

quantity between readings

19
Q

what are the 5 factors that affect rate of reaction?

A
  1. concentration
  2. temperature
  3. surface area
  4. pressure
  5. catalyst
20
Q

how does concentration affect the rate of reaction?

A

there are more reactant particles in a given volume so there are more successful frequent collisions

21
Q

how does temperature affect the rate of reaction?

A

there is more kinetic energy in the reactant particles so they move faster, therefore there are more successful frequent collisions

22
Q

how does surface area affect the rate of reaction?

A

there are more surfaces for the reactant to collide with so there will be more successful frequent collisions

23
Q

how does pressure affect the rate of reaction?

A

there is a greater chance of collisions with high pressure as reactant particles have a smaller space, therefore there will be more successful frequent collisions

24
Q

how does a catalyst affect the rate of reaction?

A

lowers the activation energy by finding an alternative pathway

25
Q

what is a closed system?

A

when no products can leave and no new reactants can enter

26
Q

what is meant by ‘yield’ in a reaction?

A

how much product you actually make in a reaction

27
Q

what is a dynamic equilibrium?

A

when the forward and backward reaction happens at the same rate

28
Q

what happens to concentration in a dynamic equilibrium?

A

stays constant

29
Q

what kind of system does a dynamic equilibrium ONLY happen in?

A

ONLY happens in a closed system

30
Q

What does Le Chatehier’s principle state?

A

Increasing temperature favours the endothermic reaction and Decreasing temperature favours the exothermic reaction

31
Q

What side does pressure favour?

A

The side with the fewest moles.

32
Q

Which catalyst is used when ammonia is produced from nitrogen and hydrogen.

A

Iron

Chemistry (13 decks)

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