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Chemistry > C8 - Rate , equilibirum and organic chemistry > Flashcards

C8 - Rate , equilibirum and organic chemistry Flashcards

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1
Q

What is the word equation for the practical about concenntration affecting rate of reaction with soidum thiosulfate solution .

A

Sodium thiosulfate solution +hydrochloric acid arrow sulfur (solid)

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2
Q

what is the product of the soidum thisoulfate solution , what state of matter is it in .

A

it i sulfur , sulfur is a solid .

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3
Q

what makes the solution is the practical go cloudy , wwhat do scientists call this ?

A

The sulfur makes the solution go cloudy , scientists call this turbidity .

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4
Q

method for the concentration practical - sodium thiosulfate

A

(recite from page )

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5
Q

is the sodium thisofulte souliton pracitcal reporucable

A

different people have different eyesights so some people may see the cross longer thn others so may not get the same results .(however is same size cross )

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6
Q

what is the second method for rp for concentration w magnesium word equation?

A

magneisum +hydrochloric acid arrow magnesium chlrodie and hyrdogen .

  • Support a gas syringe with a stand, boss and clamp.
  • Using a measuring cylinder, add 50 cm3 of dilute hydrochloric acid to a conical flask.
  • Add a 3 cm piece of magnesium ribbon to the flask. -Immediately connect the gas syringe and start a stop clock.
  • Record the volume of gas produced every 5 seconds.
  • Continue timing until no more gas is given off.
  • When the reaction is complete, clean the apparatus as directed by your teacher.
  • Repeat steps 1 to 5 with different concentrations of hydrochloric acid.
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7
Q

what does the magnesium rp for concetrtaion produce , what are we masuring .

A

hydrogen gas . so it allow us to measure the volume of hyrdogen gas produced .

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8
Q

what do both experiments for concentration show

A

show that the greater the concentration of a chemical in a reaction , the faster the reaction tkes place .

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9
Q

with both methods for rp on concentration is this finding reporudcible why ,

A

the finding is reporcuuible as the result is shown by two different experiments .

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10
Q

what does collison theory say

A

collion thoery says that chemical reactions can only take place when the reacting particles collide with eachotehr . The collisons must hve sufficent energy .

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11
Q

how is the rate of a chemical reaciton determined

A

by the frequency of sucessful collisons .

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12
Q

what is frequency

A

the number of sucessful collisons per secod .

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13
Q

on the effect of concentraiton page on star 1 what does it show and why , what abt the colliosns

A

reactions are rapid innitially because we have a large number of reactant molecules .
so have a large number of colliosns per second

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14
Q

what does the second star show , why and collisons

A

overtime reactions slow down because the numbe rof reactant molecules arw runnning out .
Meaning smaller amount of colliosn per second .

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15
Q

What does the third star show , why and collions

A

finally the reaction sotps because all of thre reactan tmolecules hve ran out .
This means the number of collisons per second is zero .

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16
Q

if the concentration of particles is doubel what does it mean in terms of collion

A

double the collisons

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17
Q

what can we say if the rate of reaction increases as we increase the concentration

A

that rate is proprotional to the conentrtion

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18
Q

look at the graph on concenrtation , how can we tell the higher concentration is a fadser reaction

A

as it is steeper than lower concentrationof reactant

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19
Q

look at the graph , how can we tell that the higgher concentration gets more product at the end

A

as we started ewith more reactatnt molecules at the start than the lower concentraiton reactant .

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20
Q

RECAP - what happens to the particles if the concentration is increases

A

more particles in the same volume

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21
Q

RECAP - collison theory if we increase the concentratoin

A

particles collide more frequenlty

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22
Q

RECAP-what happens to the rate of reaction if we increase the concentration ?

A

it increases

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23
Q

what do smaller sized blocks have compared to larger sized blocks (surface area ) what does this mean ?

A

smaller sized blocks have a greter surface area to bolume ration thn larger blocks.
This means they have more particles in the same surface , so there are more colliosns per second increasing the rate of reaciton .

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24
Q

What are the two practicals for surface area .

A

meausre the volume of co2 gas

measure the amount of co2 lost .

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25
Q

an explanaiton of measuring the volume of c02 practical surface area

A

Put ten cmcubed of hydrochlic acid into concial flask . Add calcium carbonate chips
marble chips contain the chemical calcium crbonae .
This reacts hydrochloric acid to produce carbondioxide gas which goes thorugh a delivery tube and into a measuring cylilde in a trough of water .
We can measure the volume of co2 gas and use this to determine the rate of reaction .
We can then change the surface area of the marble chips .

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26
Q

why migh measuring the volume of c02 in cylidner be noto accurate , what can we use instead?

A

measuring in a cylinder is two difficult as the bubbles are quie rpid . So use a gas syringre for m ore accurate results .

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27
Q

an explatioN for the amount of co2 lost practIal ,

A

as carbondioxide is produced the mass decreases .
Can use this to calculate the raete of reaction .
cotton wool allows the gas to escape ,
However , cotton wool also prevents acid from splashing out of the flask . If any acid did splash out , it would cause the mass to fall more than it should producing an ANOMALOUS RESULT .

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28
Q

what is the activation energy

A

is the minimum amount of energy that the particles mist have in order to react (collide succcessfully )

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29
Q

what happens to the rate of reaction if we increase the temperature

A

it increases

30
Q

what happens to the partciles if we increase temperature

A

particles have enegry greater than the reaction energy .

31
Q

collison thoery when increasing the temperature in a reaction

A

particles with the activaiton energy collide more frequenlty .

32
Q

what can we sya as the rate of reaction increases with temperature

A

the rate of reaction is proportional ot temperature till certain point , then hs no effect

33
Q

what are catalysts ?

A

catalysts increse the rate of chemical reactions but are not used up during the reaction .

34
Q

what are the advanatges using catalysts ?

A

catalysts allow us to carry out reactions quickly wihot needing to increase the temperarue saving money .

35
Q

what can we do as catalysts re not used up

A

reuse them again and again

36
Q

catalysts - look at the graph - what does the rate of reaction depend on

A

the rate of reaction depends on the n umber of particles that have enough energy to cross the activtion energy barrier and collide succesfully .

37
Q

how do catalysts increase the rate of reaction

A

catalysts increase the rate of reaction by providing a ddifferent pathway for the reaction that has a lower activation energy .

38
Q

SUM UP - how does a catalyst increase the rate of reaction (4m)

A

when a catalyst is present , the particles rewuire less energy to cross the activation energy barrier .
This mens that more particles can successfully collide per second .
Increasng the rate of reaction .

39
Q

why do we not include catalysts in the chemical equation for a reaction ?

A

As catalsts are not used up in a reaction . Catalysts are not a reactant

40
Q

what are biological catalysts called

A

enzymes

41
Q

what do all different reactions nee (enzymes)

A

different enzymes

42
Q

SUM UP -how does increasing the temperature increase the rate of reaction ? (4m)

A

Increasing the temperature increases the rate of chemical reactions as the particles have more nergy , thye move faster , this increases the frequency of collions (gretaer number of collisons per second ) .Each collison now has more energy to overcome the acitvation energy barrier and collide successfully .

43
Q

SUM UP - how does increasing the surface area increase the rate of reaction (4m)

A

increasing the surface area , increases the number of available particles , particles collide more frequenlt with activation energy , increasing the rate of reaction .

44
Q

SUM UP - how does increasing concentration increase the rate of reaction (4m)

A

increasing concentration means there are more particles in thsame volume , so particles collide more freuqnlty increasing the rate of reaction

45
Q

what is an open system

A

where substances can enter ot lrrsvrleave

46
Q

what is a closed system

A

where substances cannot enter or leave (bung in )

47
Q

in equilibrium do reactions still occur

A

yes reactions are still occuring

48
Q

what happens in an exothermic reaction , what happens to the temperature .

A

transfers energy to the surrounds , the temperature of the surroundings increases

49
Q

what happens in endothermic reactions , what happens to the temperature .

A

absorbs energy from the surroudings and the temperature of the surroundings ddecreases .

50
Q

what is dynamic equillibrium

A

when the rate of the forward reaction equals the rate of the reverse reaction .

51
Q

check your page oon effect of changing concentration on equilibrium , what happens if we increase the concentration of NO2

A

The concentration of reactions to produts is no longer at equilibrium .
The foreard and reverse reactions are not taking place at the sae rate
so the concrations of all the subsatcnes will change into equilibrium is reached . IN THIS CASE , increasing the cocnentraion of NO2 m ore N2O4 will be formed until equilibirum is reached .

52
Q

(look t equilibirum sheet ) what will happen if we decrease the concentration of N204

A

Because we have decreased the concentration of N204 , the system is no longer at equilibrium .
More NO2 will react to form N204 util the equilibrium is reached again .

53
Q

What would happen if we increase the concentration of N204 (look at equilibrium sheet )

A

As we increase the concentratgion of N204 , the system is no longer at equilibrim .
More N204 will turn into NO2 until equilibirum is reached again .

54
Q

(changing temp sheet example ) in the reaction , the forward reaction is exothermic , what does this mean ?

A

It means that energy is released and the temperature of the system increases .

55
Q

what does it mean if the reaction is exothermic one way

A

it is endothermic the other .

56
Q

(changing temp sheet example ) what is the reverse reaction and what does this mean

A

Reverse reaction is endothermic , meaning when the reverse reaction takes place , energy iss taken in and the temperature of the sysem decreases .

57
Q

changing temp sheet example ) what happens if we increase the temperature of this system

A

the equilibrium will shift ot the left to reduce the temperature .
Reverse reaction is endothermic so energy is taken in cauing the temperature to fall .
So the amount of NO2 Would increase , and the amount of N204 would decrease ,

58
Q

(changing temp sheet example )What would happen if we decrease the temperature of this system

A

Equilibrium iwll shift ot the right to increase the temperature ,
As the forwardd reaction is exothemric , so the enrgy is relased causing the temperature to increase
IN THIS CASE , the amount of N204 would increase and the amount of NO2 would decrease .

59
Q

what type of moleucles does pressure affect

A

reactions involivng gases .

60
Q

What does the pressure of a gas depend on

A

the number of molecules

61
Q

(check pressure sheet ) which container has more pressure left or right

A

the right

62
Q

what happens to the equilibrium if you increse the pressure on a reversible reaction

A

the equilibrium shifts to the side with the smaller nuber of moecules .TO minimise the affect .

63
Q

what happens to the equilibrium if you decrease the pressure on a reversible reaction

A

then the position of the equilibrium shifts to the side with thelarger number of molecules .

64
Q

(check pressure sheet ) what happens if we increase the pressure of the equilibrium for example EXPLAIN

A

The equilibrium iwll move to the right hand side as the right hand side has fewer molecules than the left .

65
Q

(check pressure sheet ) what happens if we decrease the pressure of the equilibrium for example EXPLAIN

A

if we reduce the pressure on the reaction , the equilibrium will shift to the left hand side as the left hand side has more molecules than the right/

66
Q

In terms of pressure , what happens to the equilibrium if both sides of the equation has the same number of mollecules ?

A

changing the pressure has no effect on the position of the equilibirum ,

67
Q

What hppens if we heat hydrated copper sulfate , what does this reaction produce .

A

it reacts to form anhyrdrous copper sulfate which is white . This reaction also produces water .

68
Q

what type of reaction is it if we heat hydrated copper sulfate , how can you tell ?

A

as we are heating it , we are putting energy in , this tellus us that the forward reaction is ENDOTHERMIC .

69
Q

how do we do the reverse for the anhydrous copper sulfate reaction .

A

if we take our anhyrdous copoper sulfate and add water , the reaction is reversed .

70
Q

what type of reaction is the reverse reaction for anhydrous copper sulfate , how do we know

A

in the reerse reaction , energy is released , the reaction gets hot . This tells us the reverse reaction is EXOTHERMIC .

Chemistry (20 decks)

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