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chemistry all note flashcards - 3rd And 4th > 4.3 - Rates of reaction > Flashcards

4.3 - Rates of reaction Flashcards

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1
Q

when can a chemical reaction only happen

A

if the reactant particles collide with enough energy

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2
Q

what is activation energy (Ea)

A

the amount of energy the particles need to react

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3
Q

what is the equation for rate of reaction

A

rate = collision frequency x percentage success

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4
Q

what does the overall rate of a reaction depend on

A

collision frequency - how often the particles collide with each other

percentage success - what percentage of the collisions have enough energy

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5
Q

what are the factors that affect the rate of a reaction in terms of collision frequency and percentage success

A

solid surface area - collision frequency
solution concentration - collision frequency
temperature - percentage success
catalysts - percentage success

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6
Q

why does higher solid surface area increase rate

A

-more of the solid is exposed to other particles
- so the collision frequency is higher
- so there are more successful collisions per unit time

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7
Q

why does higher solution concentration/ gas pressure increase rate

A
  • there are more particles per unit volume
  • so the collision frequency is higher
  • so there are more successful collisions per unit time
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8
Q

why does higher temperature increase rate

A
  • the particles have more kinetic energy
  • so the percentage of collisions with enough energy is higher
  • so there are more successful collisions per unit time
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9
Q

why do catalysts increase rate

A
  • they provide an alternative route with a lower activation energy
  • so the percentage of collisions with enough energy is higher
  • so there are more successful collisions per unit time
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10
Q

for solutions and gases why does increasing the concentration or pressure increase the rate

A
  • there are more particles per unit volume
  • so collision frequency is higher
  • so there as more successful collisions per unit time
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11
Q

how can you increase the concentration

A

dissolve more solute particles so there are more particles per unit volume

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12
Q

how can you increase the pressure

A

by making the reaction vessel smaller

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13
Q

what experiment explored the affect of concentration on rate

A

disappearing cross experiment

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14
Q

what can the effect of concentration on rate be demonstrated by

A

reacting sodium thiosulphate solution with hydrochloric acid

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15
Q

what is the chemical equation for reacting sodium thiosulphate with hydrochloric acid

A

Na2S2O3(aq) + 2HCl(aq) –> 2NaCl(aq) + S(s) + SO2(g) + H2O (l)

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16
Q

what is the input variable in the disappearing cross experiment

A

the concentration of the NaS2O3(aq)

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17
Q

what is the output variable in the disappearing cross experiment

A

the time taken for the cross to disappear

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18
Q

what are the control variables in the disappearing cross experiment

A

total volume of solution
concentration of HCl (aq)
temperature

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19
Q

what is rate calculated from in the disappearing cross experiment

A

time taken

rate (S-1) = 1/ time taken

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20
Q

what would the graph for the disappearing cross experiment/ concentration effect on rate look like and why

A

would be proportional and show a straight line through the origin
because the rate is proportional to concentration

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21
Q

for solids why does the surface area increase the rate

A
  • more of the solid is exposed to the other particles
  • so the collision frequency is higher
  • so there are more successful collisions per unit time
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22
Q

how is increased surface area achieved

A

by cutting or grinding up the solid

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23
Q

what experiment explores the affect of surface area on rate

A

the marble chip experiment

24
Q

what can the effect of surface area on rate be demonstrated by

A

reacting calcium carbonate chips with hydrochloric acid

25
Q

what is the chemical equation of reacting calcium carbonate chips with hydrochloric acid

A

CaCO3(s) + 2HCl(aq) –> CaCl2(aq) + H2O(l) +CO2(g)

26
Q

what is the input variable in the marble chip experiment

A

the sizes of the CaCO3(s) chips

27
Q

what is the output variable in the marble chip experiment

A

the volume of CO2(g)

28
Q

what are the control variables in the marble chip experiment

A

-mass of CaCO3(s)
- volume and concentration of the HCl(aq)
- temperature

29
Q

what is the volume of CO2 measured in, in the marble chip experiment

A

using a gas syringe or inverted measuring cylinder in water

30
Q

what does the graph of the marble chip experiment/ effect of surface area on rate look like and why

A

the line from the smaller chips has a steeper start
– because the rate has increased so volume of CO2 increases faster

both lines have the same final volume
– because the total amounts of reactants hasn’t changed so eventually produces the same amount of CO2

31
Q

why does increasing temperature increase the rate

A
  • the particles have more kinetic energy
  • so the percentage of collisions with enough energy is higher
  • so there are more successful collisions per unit time

although particles also collide more often the effect is not significant

32
Q

how can increasing temperature be accomplished

A

by heating

33
Q

what experiment explores the effect of temperature on rate

A

magnesium and acid experiment

34
Q

what can the effect of temperature on rate be demonstrated by

A

reacting magnesium with hydrochloric acid

35
Q

what is the chemical equation of reacting magnesium with hydrochloric acid

A

Mg(s) + 2HCl(aq) –> MgCl2(aq) + H2(g)

36
Q

what happens in the magnesium and acid experiment

A

the magnesium disappears

37
Q

what is the input variable of the magnesium and acid experiment

A

the temperature of the HCl (aq)

38
Q

what is the output variable of the magnesium and acid experiment

A

the time taken for Mg(s) to disappear

39
Q

what are the control variables in the magnesium and acid experiment

A

mass and surface area of Mg(s)
volume and concentration of HCl(aq)

40
Q

how can rate be calculated in the magnesium and acid experiment

A

time taken

rate (S-1) = 1/ time taken

41
Q

what would the graph of the magnesium and acid experiment/ effect of temperature on rate look like and why

A

curve upwards
not a straight line
– because rate isn’t proportional to temperature

doesn’t go through the origin
–because the rate isn’t 0 at 0 degrees

42
Q

what are catalysts

A

usually solids which
- increase rate
- remain chemically unchanged

43
Q

how do catalysts work

A

they increase rate because
- they provide an alternative route with a lower activation energy
- so the percentage of collisions with enough energy is higher
- so there are more successful collisions per unit time

44
Q

what experiment explores the effect of catalysts on rate of reaction

A

hydrogen peroxide experiment

45
Q

what can the effect of a catalyst on rate be demonstrated by

A

using the decomposition of hydrogen peroxide

46
Q

what is the chemical equation for the hydrogen peroxide experiment

A

2H2O2(aq) –> 2H2O(l) +O2(g)

47
Q

why are catalysts not in the reaction equation for the hydrogen peroxide experiment

A

they are uchanged during the reaction

48
Q

what is the speed of the reaction in the hydrogen peroxide experiment without a catalyst

A

very slow, takes days to finish

49
Q

what is the catalyst in the hydrogen peroxide experiment

A

manganese(IV) oxide (MnO2) - which is a black solid

50
Q

what is the speed of the reaction in the hydrogen peroxide experiment with a catalyst

A

takes place much faster, takes only a few seconds to finish

51
Q

how can you measure the effectiveness of catalysts

A

comparing how they affect rate

52
Q

what is the input variable in the hydrogen peroxide experiment

A

which catalyst is being used

53
Q

what is the output variable in the hydrogen peroxide experiment

A

volume of O2(g)

54
Q

what are the control variables in the hydrogen peroxide experiment

A

volume and concentration of H2O2(aq)
temperature
mass and surface area of catalyst

55
Q

what would the graph of the hydrogen peroxide experiment/ how catalysts affect rate look like and why

A

more effective catalysts increase rate more effectively which results in a steeper line on the graph

the initial amounts of reactants is the same so all lines would flatten out eventually at the same volume of oxygen if you waited long enough

chemistry all note flashcards - 3rd And 4th (13 decks)

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