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GCSE Chemistry Revision > C6 - Rates Of Reaction - Needs Work > Flashcards

C6 - Rates Of Reaction - Needs Work Flashcards

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1
Q

What is a formulation

A

Mixture where components have specific purposes combined to make a useful product

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2
Q

Give 2 things needed for a chemical reaction to take place

A

Collision in the correct orientation
Sufficient activation energy

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3
Q

What is activation energy?

A

Minimum amount of energy needed for a chemical reaction to happen

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4
Q

What is the rate of reaction

A

Time taken for reactants to be used up/formulation of products etc

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5
Q

Give 4 things that affect rate of reaction

A

Temperature
Surface area
Catalysts
Concentration/pressure

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6
Q

How does temperature affect rate of reaction?

A

Increasing temperature gives particles more kinetic energy
Increases frequency of successful collisions
Rate of reaction increases

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7
Q

How does increasing surface area increase rate of reaction

A

Leads to more particles exposed
Increases frequency of successful collisions
Rate of reaction increases

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8
Q

How do catalysts increase rate of reaction

A

Provide a different pathway for the reaction to take place with a lower activation energy
Increase rate of reaction

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9
Q

How does increasing concentration/pressure increase rate of reaction

A

More particles in a specific volume
Increases frequency of successful collisions
Rate of reaction increases

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10
Q

Never write fractional answers when drawing tangents - only decimals

A
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11
Q

What is a reversible reaction

A

A reaction where there is a forward and backward reaction taking place at the same time

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12
Q

In a reversible reaction, one reaction is __ and the other is ____

A

Exothermic
Endothermic

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13
Q

What is dynamic equilibrium?

A

Rate of forward and backwards reactions are equal
So concentrations of reactants and products are constant (NOT AMOUNTS)

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14
Q

What type of system does dynamic equilibrium take place in?

A

A closed system

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15
Q

How can you create a closed system in an experiment

A

Lids on beakers

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16
Q

If temperature is increased which side (exo or endo) does equilibrium shift to (in an exam say left or right)?

A

Endothermic

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17
Q

Why does equilibrium shift to the endothermic side if temperature is increased

A

Rate of endothermic reaction increases - to counteract the effect of rising temperature I think?

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18
Q

Where does equilibrium shift to if pressure is increased?

A

To the side with the least moles
Yield on the side with the least moles increases (presumably the rate of the reaction towards this side increases therefore?)

19
Q

What does the haber process do?

A

Method for the industrial production of ammonia

20
Q

What is the forward reaction in the haber process

A

Exothermic

21
Q

What is the reaction for the haber process

A

(g)N2 + 3H2(g) <=> 2NH3(g)

22
Q

Give 2 ways the rate of reaction is I ncreased

A

Iron catalyst
High temperature

23
Q

Why is temperature decreased

A

To increase Exothermic (forward) direction yield - increase ammonia yield

24
Q

Why is pressure increased

A

Increase yield on the side with fewer moles (ammonia side)

25
Q

What pressure is the haber process done at?

A

200 atmospheres

26
Q

What temperature is teh haber process done at

A

450 degrees

27
Q

Remaining hydrogen and nitrogen from the haber process is ___

A

Recycled

28
Q

On cooling, ___ ammonia is removed

A

Liquid

29
Q

Give the method for measuring rate of reaction by measuring volume of gas produced

A
  1. Measure 50 ml of HCl into a conical flask using a measuring cylinder
  2. Add a 1g strip of magnesium into the conical flask
  3. Start the stopwatch and record volume of gas release using a gas syringe every 10 seconds for 1 minute
  4. Ploy results on a graph of product formed over time and find the gradient to calculate rate of reaction
    R. Repeat with different acid concentrations
30
Q

Give a method for finding rate of reaction by checking for colour change

A
  1. Measure 50 ml of sodium thiosulfate solution into a conical flask with a measuring cylinder
  2. Place the conical flask on top of a printed black cross
  3. Measure 20ml HCl Ito a test tube and heat to 40 degrees with a water bath
  4. Add teh HCl, swirl and start the timer
  5. Time how long it takes for the cross to disappear by looking from above
  6. Repeat for other temperatures of HCl
  7. Plot a graph of temperature of reactants and rate of reaction (how long it took)
31
Q

What was the traditional fertiliser

A

Manure

32
Q

Give 3 things used in NPK fertilisers

A

Nitrogen
Phosphorus
Potassium

33
Q

Give 3 ways NPK fertilisers benefit food production

A

Growing tastier and bigger and enhances productivity

34
Q

How is nitrogen made

A

Made from ammonia from haber process

35
Q

Give stages of forming ammonium nitrate

A

Haber process
Ammonia formed
Ammonia used to make nitric acid
React nitric acid with more ammonia to make ammonium nitrate fertiliser

36
Q

Give a way ammonium nitrate is formed

A

Ammonia from haber process reacted with sulfuric acid

37
Q

How is phosphorus obtained

A

From mined phosphate rock

38
Q

Why can’t phosphate rock be used as a fertiliser?

A

Its insoluble

39
Q

How is phosphorus made into a fertiliser?

A

Treated with nitric acid/Sulfuric acid to make a soluble salt for fertiliser

40
Q

In what two forms is mined potassium found in

A

KCl or K2SO4

41
Q

If energy change is positive in the forward direction, this reaction is endo/Exothermic?

A

Endothermic

42
Q

what is rate of reaction measured in

A

g/s or cm cubed/s or mol/s

43
Q

give 4 things affecting rate of reaction

A

pressure of reacting gases
surface area of solid reactants
temperature
presence of catalysts

44
Q
A

GCSE Chemistry Revision (13 decks)

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