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8/9/2019 14 Chemical Kinetics
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1. What is the efect o catalyst on rate constant? [1]
2. How is activation energy afected on adding a catalyst? [1]
3. What do you mean by the term collision re!uency? [2]
". How does collision theory e#$lain ormation o $roducts in a chemical
reaction? [1]
%. What is the drawbac& o collision theory? [2]
'. How does the number o collisions change on increasing the tem$erature? [2]
(. )here is no bar on the no. o collisions among the reaching s$ecies. Why most
o the reactions do not ta&e $lace under normal conditions? [2]
*. +rom the ,g. -1 [2]
-a /alculate 0 or the reaction activation energy or orward reaction.
-b dentiy the curve or catalysed reaction.
-c what is the energy o activation in the $resence o catalyst?
4. )he activation energy o reaction is (%.2 567mol in the absence o a catalyst
and %8.1" 5679ol in the $resence o a catalyst. How many times will the reaction
grow in the $resence o a catalyst i the reaction $roceeds at 2%8/? [2]
18. )he rate o a $articular reaction !uadru$les when the tem$erature changes
rom 243 5 to 313 5. /alculate activation energy or such a reaction. [2]
1. :ive an e#am$le o $seudo ; ,rst order reaction ? [1]
2. Write the e#$ression or hal ; lie $eriod o a ,rst order reaction? [1]
3. < ,rst order reaction is ound to have a rate constant 5 = %.% > 181" sec 1.
+ind hal lie o reaction? [1]
". )he time re!uired to decom$ose @2/l2 to hal o its initial amount is '8 min.
the decom$osition is a ,rst order reaction calculate the rate constant o the
reaction? [2]
%. )he rate constant or the ,rst order decom$osition o A2@% at 2%8/ is 3B182
min1. t the initial concentration o A2@% is 2B183 mol7C How long will it ta&e
to dro$ the concentration to %B18" mol 7C ? [2]
'. Write
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tem$erature range24%5 to 38%5 what would be the activation energy or this
reaction? -E=*.31"6&1 mol1 [3]
4. )he rate constant or a reaction is 1.%> 18( s1 at %88/ and ".%> 18( s1at
1888/. /alculate the value o activation energy or the reaction E=*.31" 651
mol1? [3]
18. Flot a gra$h showing variation o $otential energy with reaction .coordinate?
[1]
1. < catalyst increases the rate constant value.
2. < catalyst lowers the activation energy by ollowing a diferent $ath or the
reaction.
3. )he no. o collisions $er second $er unit volume o the reaction mi#ture is&nown as collision re!uency. t is denoted by G.
".
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'. )he reaction 2A2@% -g K2A@2 -g J@2 -g was studied and the ollowing data
were collected M s.no [A2@%] mol C1 Eate o disa$$earance o [A2@%]-mol7C7min
1. 1.13>182 3">18% 2. 8.*" >182 2%>18% 3. 8.'2>182 1*>18%
Netermine i )he order ii )he rate law. iii Eate constant or the reaction. [3]
(. )he ollowing e#$erimental data was collected or the reactionM /l2 -g J 2A@
-g K 2 A@/l-g )rial ntial conc. @ /l2 -mol7C [A@] mol7C nitial Eate-mol7C7s
1 8.18 8.818 1.2 B 18"
2 8.18 8.838 18.* B 18"
3 8.28 8.838 21.' B 18" /onstruct the rate e!uation or the reaction. [3]
*. Nraw a gra$h or a /oncentration o reactant against time or a Dero order
reaction. b Cog [Eo]7 [E] against time or a ,rst order reaction. [2]
4. What is the use o integrated rate e!uation? [2]
18. +or ,rst order reaction ; < KL Write -1 Niferential rate law. -2 ntegrated
rate law.
1. Hydrolysis o ethyl acetate when concentration o water is very large is an
e#am$le o $seudo ,rst order reaction.
/H3/@@ /2H% J H2@ K /H3 /@@H J /2H%@H.
2. +or a ,rst order reaction the hal lie $eriod is )172 = 8.'43&
'. 18" s1 [1]
2. /onsider the e!uation 2 A@ -! J 2H2 -g K A2 -g J 2H2@ -g )he rate law
or this e!uation is ,rst order with res$ect to H2 and second order with res$ect
to A@. write the rate law or this reaction. [1]
3. )he rate Caw or the reaction 18% 2. 8.*" >182 2%>18% 3. 8.'2>182 1*>18% Neterminei )he order ii )he rate law. iii Eate constant or the reaction. [3]
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(. )he ollowing e#$erimental data was collected or the reactionM /l2 -g J 2A@
-g K 2 A@/l-g )rial ntial conc. @ /l2 -mol7C [A@] mol7C nitial Eate-mol7C7s
1 8.18 8.818 1.2 B 18"
2 8.18 8.838 18.* B 18"
3 8.28 8.838 21.' B 18"
/onstruct the rate e!uation or the reaction. [3]
*. Nraw a gra$h or a /oncentration o reactant against time or a Dero order
reaction. b Cog [Eo]7 [E] against time or a ,rst order reaction. [2]
4. What is the use o integrated rate e!uation? [2]
18. +or ,rst order reaction ; < KL Write -1 Niferential rate law. -2 ntegrated
rate law. [2]
1. a ince the units o rate constant are Cmol1 s1 )he reactions is o second
order. b ince the units o rate constant are s1 )he reaction is o ,rst order.
)he rate o reaction increases eight times.
(. @rder o A@ is 2 Eate law = 5 [/l2] [A@]2
4. Ose o integrated rate e!uation
1. )he value o rate constant can be &nown when concentration o reactant at
diferent times are &nown
2. @rder o a reaction can be determined by the &nowledge o reaction
concentration atdiferent times.
1. s rate o reaction always constant? [1]
2. nlist the actors afecting rate o a reaction? [1]
3. What do you understand by rate law e#$ression? [2]
". s it $ossible to determine or $redict the rate law theoretically by merely
loo&ing at the e!uation? [1]
%. Ne,ne the terms ; i @rder o a reaction [2] ii 9olecularity o a reaction.
'. What are elementary and com$le# reactions? [2]
(. Niferentiate between order and molecularity o a reaction? [2]
*. Netermine the overall order o a reaction which has the rate law [2] E = 5
[
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18. +or the reaction
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%. What is instantaneous rate o a reaction? How is it determined? [2]
'. +or the ollowing reactions write the rate o reaction e#$ression in terms o
reactants and $roducts? [2]
i "AH3 -g J %@2 -g K "A@ -g J 'H2@ -g ii 2A2@% K 2A@2 J @2
(. +or the chemical decom$osition o @2/l2 its initial concentration is 8.*"28
mol7C and ,nal concentration is 8.21% molC1 in 2 hours. What is the average
rate o this reaction? [2]
*. n the e#$ression o rate o reaction in terms o reactants what is the
signi,cance o negative sign? [2]
18. < chemical reaction 2< Q "LJ/ in gas $hase occurs in a closed vessel. )he
concentration o L is ound to be increased by % B 183 mole C1 in 18 second.
/alculate -i the rate o a$$earance o L -ii the rate o disa$$earance o