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chemistry 1st mock > rates of reaction (4.1) > Flashcards

rates of reaction (4.1) Flashcards

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1
Q

when can a chemical reaction only happen

A

when the reactant particles collide with enough energy

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2
Q

what is the amount of energy particles need to react called

A

activation energy

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3
Q

what does the overall rate of reaction spend on

A

the collision frequency
percentage success

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4
Q

what is a collision frequency

A

how often do the particles collide with each other

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5
Q

what is a percentage success

A

what percentage of the collisions have enough energy

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6
Q

what are the four factors that effect rate of reaction

A

surface area
concentration
temperature
catalysts

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7
Q

why does a higher solid surface area increase rate of reaction

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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8
Q

why does increasing temperature increase rate of reaction

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 does having a higher concentration/pressure increase rate of reaction

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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10
Q

why do catalysts increase rate of reaction

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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11
Q

what experiment shows the effect of surface area with rates of reaction

A

the marble chip experiment

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12
Q

what is the marble chip experiment

A

reacting calcium carbonate (marble) with hydrochloric acid

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13
Q

indépendant variable of the marble chip experiment

A

sizes of CaCO3(s) chips

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14
Q

dependant variable of the marble chip experiment

A

volume of CO2(g)

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15
Q

control variable of marble chip experiment

A

mass of CaCO3(s)
volume and concentration of HCL(aq)
temperature

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16
Q

results of marble chip experiment

A

faster beginning because the rate is increased, so the volume of CO2 is increasing faster
same final volume brace the amount of reactants hasn’t changed, so the experiment produces the same amount of CO2

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17
Q

what experiment is used to show how concentration effects rate of reaction

A

disappearing cross experiment

18
Q

what is the disappearing cross experiment

A

reacting sodium thiosulphate solution with hydrochloric acid

19
Q

independent variable of disappearing cross experiment

A

concentration of the NaS2O3 (sodium thiosulphate solution)

20
Q

dependent variable of disappearing cross experiment

A

time taken for cross to disappear

21
Q

control variables for disappearing cross experiment

A

total volume of solution
concentration of HCL(aq)
temperature

22
Q

1 rate =

A

collision frequency x percentage success

23
Q

how is rate calculated in the disappearing cross experiment

A

rate = 1/time taken (s)

24
Q

what does the disappearing cross experiment show

A

rate is proportional to concentration
double the concentration = double the rate
triple the concentration = triple the rate etc

25
Q

what experiment is used to show how temperature effects rate of reaction

A

magnesium and acid experiment

26
Q

what is the magnesium and acid experiment

A

when you react magnesium(s) with hydrochloric acid(aq)

27
Q

indépendant variable for magnesium and acid experiment

A

temperature of HCL(aq)

28
Q

dependant variable for the magnesium and acid experiment

A

time taken for the Mg(s) to disappear

29
Q

control variable for the magnesium acid experiment

A

mass and surface area of MG(s)
volume and concentration of HCL(aq)

30
Q

how is rate calculated in the magnesium and acid experiment

A

rate = 1/time taken (s)

31
Q

what does the magnesium acid experiment show

A

rate isn’t proportional to temperature

32
Q

what are catalysts

A

substances that increase rate and remain chemically unchallenged

33
Q

how do catalysts work?

A

they provide an alternate 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

34
Q

what experiment shows the effect of catalysts with rate of reaction

A

hydrogen peroxide experiment

35
Q

what is the hydrogen peroxide experiment

A

the decomposition of hydrogen peroxide

36
Q

what is the catalyst used in the hydrogen peroxide experiment

A

manganese(IV) oxide (mnO2)

37
Q

what does manganese oxide do in the hydrogen peroxide experiment

A

it makes a reaction that usually takes days to finish, take only a few seconds to finish

38
Q

independent variable in the hydrogen peroxide experiment

A

what catalyst is being used

39
Q

dependent variable of the hydrogen peroxide experiment

A

volume of O2

40
Q

control variables in the hydrogen peroxide experiment

A

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

41
Q

what does the hydrogen peroxide experiment show

A

more effective catalysts increase rate more effectively

chemistry 1st mock (10 decks)

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