Module 3.2 THIS IS CHEM

Question 1

Collision theory
-in order for prticles to react what must they do ?

Answer 1

They msut collide .
-if particles do not collide , then they cannot react .

Question 2

What happens when partilxes react ?

Answer 2

When particles react, chemical bonds must be broken. (This required energy is the activation energy >)
-So in order, for a reaction to happen, particles must collide with enough energy to start breaking the chemical bond.

Question 3

what happens if the collision does not hve enough energy >

Answer 3

Particles cannot react .
-Instead they simply bounce off eachother .

Question 4

What is the htird way in which for a reaction take place?

Answer 4

parciles must colllide in the COORECT ORIENTATIOin .
-the rat eof reaction is PROPROTIONAL to thenumber of effective collisions per second - frequency of cells .

Question 5

One way to increase the rate of reaction is to increase the concentration of the reactants.
-explain this using collision theory.

Answer 5

a higher concentration , means we have more reactant particles int he same volume .
-as the reactant partciles are closer together ,w e have an increased chanc eof collisions taking place - increased freqency of collions .
-some of thee colliosns will be effective leading to rwzction .
-this means rate of reaction will increase .

Question 6

Explain the rate of reaction in gases and how to increae it .

Answer 6

We can increase the rate of reaction by increasing gas pressure.
-Incresing the pressure, makes particles closer together.
-Increasing the frequency of collisions leading to an increased rate of reaction.

Question 7

check sheet for the equation
what can we measure when measuring the rate of reactnt ?

Answer 7

-how quickly he amount of reactant decreses .
-OR how quickly , the amount of produc is formed , this depens onw ht is esiser to measure accurately .

-in reaction , making co2 , measuring volum eof gas is straightforward .

Question 8

two ways of measuring the volume of gas .

Answer 8

-one way is to catch the gas in an upturned measuring cylinder .

-the other way is a more accurtae way which is a gas syringe .
–however , in oth ways ,w e can red the volume of gas at regular intervals fromt he scar .

Question 9

check sheet , explain star one

Answer 9

initially , as we get a lot of product formed rapidly . This is telling us that the rate of reaction is fast .
-as w ehave a high cocnenration of reactants and a high frequency of efective collisions .

Question 10

check sheet explain star two

Answer 10

Over time, the reaction slows down ,a s the hydrochloric acid is reacting .
-so the concentration of hcl is decreses and hcl is a LIMITING RECTANT, therefore the frequency of effective colliosions is reduced .

Question 11

check sheet , explain star three

Answer 11

evenutally , the reaction stops and more product is formed as a result , all the hcl has reacted and there is no m ore effective collsions .

Question 12

rate of reaction at any point is shownn by what ?

Answer 12

drawing a tangent on the graph .
units could be cm3/s –> dependsss thooo .

Question 13

Recap for a reaction taking place

Answer 13

-for a reaction to take place reactant particles must collide in the correct orientation .

Question 14

what two things must particles collide with for a reaction to take place ?

Answer 14

The reactant particles must also collide with enough energy to start breaking the chemical bonds in the reaction . aka as activation energy .

Question 15

what is activation energy

Answer 15

activation energy is the minimum energy particles must have in order to start a reaction by breaking chemical bonds .

Question 16

during any reaction , what must happen to the chemical bonds ?

Answer 16

chemical bonds must be broken and new chemical bonds must be formed .
check sheet for two moelucles a-b and c-d .

Question 17

check the sheet to see the bonds being broken and forming as well .
-what happens to the two molecules .

Answer 17

-as the two molecules collide there comes a point where the existing chemical bonds are in the process of breaking and in the process of forming .
-scientists call this the transition state .

Question 18

what happens in the transition state ?

Answer 18

the transition state is unstable and goes on to form the products .
-check sheet to check the graph .

-On this graph you can see that the activation energy is the difference between the highest point on the curve and reactants .

Question 19

On the graph , what does the highest point on the curve represent ?

Answer 19

the transition state.

Question 20

Now ,a s we know about transition states , we can add a bit more to our activation energy definition .

Answer 20

the activation energy is the enthalpy difference between the reactants and the transition state .

Question 21

check graph to see two exothermic reactions which i have labelled one and two .

-explain graph one

Answer 21

graph one has a relatively low activation energy .
-So the reaction could take place quite rapidly at room temperature .

AS , at room temperature , there is a relatively large proportion of reactant molecules will collide with enough energy to cross the activation energy barrier and react .

Question 22

explain graph 2

Answer 22

graph 2 , has a relatively high activation energy ,.
-This means that a room temperature ,t his reaction should be , relatively slow , as now only a smaller proportion of reactant molecules will collide with enough energy to cross the activation energy barrier .

Question 23

How does a catalyst increase the rate of reaction ?

Answer 23

A catalyst allows the reaction to take place via an alternative pathway with an alternative pathway with a lower activation energy than an uncatalyzed reaction .

Question 24

what is the effect without a catalyst

Answer 24

higher activation energy , meaning particles collide with a large amount of energy to form the transition state and react .
-This means a small proportion of particles have enough nervy to cross the activation energy barrier , so the rate of reaction is relatively low .

Question 25

-This means ,t hat a greater proportion of particles will collide with enough energy with enough energy to form he transition state and react .

Answer 25

-In this case , the rate of reaction will be greater than without a catalyst .

Question 26

What is the key thing about catalysts ?

Answer 26

Catalysts are not used up in a reaction and are not permanently changed , therefore catalysts can be reused.

Question 27

What is the purpose of using a catalyst ? -give some economic benefits and environmental benefits

Answer 27

-By using a catalyst , we can make reactions take place more rapidly , even at relatively low low temperatures . -This reduces the amount of energy needed by the chemicals itself . -which in then reduces the need to burn lots of fossil fuels , to provide this energy , this saves money providing an economic benefit . -this also reduces carbon dioxide emissions make the chemical industry more sustainable .

Question 28

What is a disadvantage for catalysts ?

Answer 28

some catalysts are toxic , so this is a negative impact , needs to be weighed against the benefits .

Question 29

We can divide catalysts into two categories , what are they ?

Answer 29

Hetrogeneous ctlaysts -Homogeneous Ctalysts

Question 30

What are hetereogenous catalystistd

Answer 30

they have a different physcal state (phase) to the reactants .

Question 31

Whatgenoeus catlaysts

Answer 31

thery are int he same physical satae ([ahse0 as the reactants

Question 32

e are homog

Question 33

give an example of hetrogeneous catlaysts and check the sheet

Answer 33

-In the haber porcess , the gases nitrogen and hydrogen react together tof orm the gas ammoni . -the catalyst int his reaction is iron which is a solid . -as the catlaysgts is ain a different physical state then the reactions it is an exmpale of hetrogenous catlayst .

Question 34

how a hetrogenous ctalyst woks -there are two steps adsorption a nd desoprtion

Answer 34

...

Question 36

stage 1 of hetreogenous catlayst

Answer 36

reactant moelcules form weakbonds with the surface of the catalyst . -scientists call the first stage adsoprtion ADSOPRTION NOT ABSORPTION .

Question 37

stage 2 of heterogenous catalyst

Answer 37

second sage reaction takes place to form the [porducts . -in the final stage porduct moeleucues are released from the surafce of the catalyst . -scienitsts call thie final stage desoprtion .

Question 38

homogenous catlaysts same pahse as the reacion check sheet for the ecample

Answer 38

-oe of the reactions repsoinsible for ozonde destruction int he aormpsopehre . -ozone is converted into oxyge , this reaction is catalsyedb y a chlorine radical . -both reactant and altalyst are in gases so it is a hoogenous atlast .

Question 38

Examples of hetrogenous catlayst

Answer 38

-we often see reactions with the gaseous reactants and a solid catlayst . -moreover ,w e could also see htereogenous catlaysts with liquid reactants and a solid catalyst .

Question 39

key about the homogenous catalsy

Answer 39

in homogenous catalsyts the catalyss reacts with the reaction to form an intemrediate . -reaction shown (zone0 are sonsits of two tages . -catalyst forms an itnemrediate in syage 1 -stage 3 , intermediste rects sagain and the catalyst is renewed .

Question 40

if we measure the energy of all the moelcules in a gas , liquid or solution we egt a curve

Answer 40

this curve is the maxewell boltzman distrubtion curve .

Question 41

key point one of the maxwell distrubtuion curgve

Answer 41

the cruve starts at 0___0 aka the origin . -wht htis means is that htere are no moelcules with zero energy

Question 42

second key point about curve , check star one

Answer 42

some moelcules have avery high energy , in fc , one does does not ouch the x axis at highe negries . -telling us ther eis no maximum energy that the moeclules could have .

Question 43

key point threee about the curve

Answer 43

-the area under the curve tells us the total number of moelcules in the suytem .

Question 44

key point 4 baout the curve ,c heck star two

Answer 44

check str two - the most probabale enegry is directly under the pek of the curve . -BUT tsra three --- ? but the mean energy is slightly to the right of this .. -Thsat is ecuae the particles at very high energy skew the mean to the right .

Question 45

key point about five , star four

Answer 45

activarion enegry , remeber in order to collide effectively and reax . -moelcules must have at least this energy -thes emoeluelces are represented by the re under the curve shadedb lude to th right of the activtion energy

Question 46

-what does a ctalst do , to the maxwell boltzman curve

Answer 46

catalysts porvidean alternative patheay with a lwoer acitviaiton enegry , the energy line is ec with a catalyst . -all of the moelcules which now at least have this energy ec , cn collide efectively and rect . -shown by the area under the curve being much greater tnumebr of meocluels comaped to the uncatalsyed line therefore , expalinw hy rof highw a calas .

Question 47

another ay rof reaction increase ss by increasing the temperature what is he effect of this on the curve ?

Answer 47

t1 is the normal temp t2 is the icnrease int emp

Question 48

increase in temperature effect on the curve )1_

Answer 48

-you will notivce , that at veyr high temoeratye rtere are more aprtuces wuth a very high eenrgy . **can also see thag he MOST PORBABLE NEEGRY increases , but the number of partivcles witht he MOST PROBABLE energyf alls .

Question 49

increase in temperautre effect on the curve t2 .

Answer 49

rememebrr , are aunder the curv = the total nmber of meolcuels do not change number of meoclues . -we have any increased temp aso area sdoes not change . --so at high temp the curve shifts to the right , but height of peak falls .

Question 50

there are two effects of increasing the temperature .

Answer 50

-moelcules move faster ,s o frequency of all collisons increases . -at higher tempratue , we can see the number of meocluels with at least ctivation energy has increased substantiall . -therefore a mean greater rproptoion of the collisons are effect resulting in the rate of the reaiton to icnrease .

Question 51

combustion f metahne

Answer 51

is an example of an irreverisble reaction .

Question 53

example of a reverisble reaction check sheet

Answer 53

haver osc process , reverisble rreactions as the products are able to convert bck into the reactants . -ireverrisble arrow - a reerisble rectant tht can reach equillirbium .

Question 54

What happens in a closed sytem ?

Answer 54

no atoms can enter or leave the systme . star one - at the start if the reaction ,w e have a high cocnentration of reactants and no produtcs . -as we have a higher cocnentration of reactants ,t hue rae of the forwrd reaction is very high . -as there is no prodcuts the rate f reverse reaction is zero . -star two ma s tge frorward reaction oriceeds tge coocnetraiton of reaction decreases , cocn of poducs increse ,r ate of rvers eincrese r ate of forwrd decreses .

Question 55

star three of the clsoed sytem graph

Answer 55

eventually ,t here comes a point , where both the rte of the foreard reaction and reverse reactiona re talking place at the sme rate . -at this point ,t he cocnentration of both reactants and products remian constnt stop chanign ) so the reaction has reached equilirbrium .

Question 56

key point 1 fo the clsoed sytem

Answer 56

when we reach equillibrim , the forward and resvere reactions have not stopped -both the forward and reverse reaction are sitll taking plac but at the sme rte whch is wh y the conc of both is constant . S BOTH ARE STILL TAKING LACE - scienitnits cll this dynamic equlibrium .

Question 57

key point 2 of the closed sytem

Answer 57

-at equlllirium , cocnentrarion of both reactants and porducts are no longer chnign . -but does not mean cocnentration of both are the sme . dtar four of the taph ,we cn see a greater conc of reactants and vice vera . apslo equlibrium n e apporahced form either side , ljsut procudcts nor eactant sam conditions .

Question 58

what does the position of the eequilibrium tell us ?

Answer 58

-it tells us where the equilibrium lies torrd the rectants or products , in some cases , both are the same so equilibrium does not change .

Question 59

how can we change the po ?soiton of equlirbium

Answer 59

one way is to change the cpncentration

Question 60

what does le chateiliers pirncipe sgtae ?

Answer 60

where an external change i applied to a sytem , at equillibriu , the equillibrium moves int he rdirection to reduce the effect of the change , . -apply this to trh exmaple equation .

Question 61

apply this concept to the reaction shown on sheet , in terms of concnetration

Answer 61

-if we increase the cocnentrtion of reactnt a , as we have more meolcules off a , we have applied an external chnage to the system . -so the equillibrium now iwll move to the right to minimse the change , as the rate of the forwrd reaction is NOW greateer than the rate of the erverse reaction . -evenutallyt he rates will be the same , and we will reach a new equillirbim .

Question 62

le chartielleir princiipe ad the haber bosch procss example reaction ?

Answer 62

-nitorgen and hydroegen react tof orm ammonia , xn LO coneve ammonia backt o ammonia as it is a reverisble reaciton . by changig

Question 63

what is agas pressure porotional to

Answer 63

gas pressure is propootional to the number of gaso moelcules present . -equillobrium wills hift ot hte idse with fewer moelcules or mvore depending onw hat hte change is that needs to be couminimised . -if we icnreas epressure ,e qullibrium will shit to ehe irgt had side as there are fewer moeclues .. -pressure will only affecte quilirbum if there is a differenc ein the numbe orf moles on both sides .

Question 64

Many reversible reactions are relatively slow at room temperature . -what is the solution to this >

Answer 64

-so we often use a calasy to icnrwase the rate of reaciton KEY ; catlasyts increse the rate of botht he forward and reeverse rection by the same amount ,s o catlays hae NO EFFECT ont he position of hte eeuillibrium . -using a ctalsys means raction reches equilllibrium faster then if we ddid not use a catalsyt .

Question 65

-HOw can qwe quanitfy the position of the equillibrium ?

Answer 65

by calcualitng the equillibirum contant kc check the sheet . -imagine we have a reaction in which the reactans produce a to d . -the lwoer case numbers sohow the balancing euqaitons and have reached equilibirum .

Question 66

do the first quesiton what do u need to notice aoout this equaiton

Answer 66

-sall the reactan and porduct are gases aka the same pahse so it is a homogous equillibirum , check the sher how to do this

Question 67

what are the values in the equationa nd what is the unit for them .?

Answer 67

concentration unit is moldm-3 -cgecj tge sgeet si see giw ti work out units . -as all the units cancel out in this reaction so kc has no units .

Question 68

what does equilibirum constanr depend on ?

Answer 68

it depends on temperature . -so for the same rection , but different kc temperautre was used in different that why different k

Question 69

what does the size of the euilbirum show ? -show all the variation

Answer 69

gives us an idea of the relaitve proprotions of the reactants and products at equillirbirum -kc+1 equillibrium lies mdiway between reactants and pordcts . if kc is less than 1 + eeulliirum lies towards the reactant . -if kc is more than one equillibirum lies toward poerducts .

Question 70

what is the temperture used fed for the haber bosch process

Answer 70

althogh a low temperature should produce a high equliirum yield , the reaction owudl take place at a very low rte , so the n2 h2 moelcuels will not have enough energyt oc ross the acitivation egery barries . -therefore the tmeerature imust be high enough to alow the reaction to proceed at relisitc rite will still producing an acceptabel equilibrium yield . -a tmeperture of 200-500 degrees is used .

Question 71

what should the pressure be for the haber bosch process ?

Answer 71

a high presure increses the cocnentration og the gses , incresing the reaction rate , so high presure should produce a igh equlirium yeild and hibghr ae , however , large quantitie sof energy iwll be needed dding to cotss , d it will cause sfety ipactuis , -so to make sure workforce is not put in danger and reduce cots a pressure of 200 atmpsheres re usd .

Question 72

effect of usian iron catalyst for the haber bosch process

Answer 72

an iron catalyszciton allowing the equillibriumt o be estbalsihed agsyet nd leow temperatures to be used . Less enegry is needed to genrta eheat ,r educing ocsts .