cstr joe's
TRANSCRIPT
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ABSTRACT
This Continuous Stirred-Tank Reactor experiment which commonly known as CSTR is
conducted to observe the order of the saponification reaction and also to find the rate
constant. This experiment is conducted by mixing two different solution which is Ethyl
cetate and Sodium !ydroxide "#a$!% with e&ual volume using Continuous stirred-tank
reactor. The sample of mixed solution is then mixed with !Cl after ' minutes and titrate with
(.) * #a$!. The amount of #a$! used by the titration will be recorded for the result of the
experiment. The same procedure for the next sample will be conducted repeatedly with
continuous time taken which is )(+ )'+ ,( and ,' minutes. ifferent flowrate are been
adusted for each time taken in this experiment that is (.)(+ (.)'+ (.,(+ (.,' and (./( 01min.
ll the data are collected for the result. 2ased on the calculation and graph that have been plotted from the result obtained+ we can determine the rate of the reaction. The temperature is
fixed for the residence temperature that have been calculated in our calculation which is /( C
due to limited time to conducting the second experiment which varying the temperature.
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INTRODUCTION
Chemical reaction and reactor design are important in producing almost all in industrial
chemicals. The selection of a reaction system that operates in the safest and most efficient
way is the key to success or failure of a chemical plant. Reactor is the e&uipment that changes
the raw materials to the product that we want. good reactor will give a high production and
economical. $ne of criteria to design or to choose a reactor knows the effectiveness of the
reactor itself. There are many reactors depending on the nature of the feed materials and
products. $ne of the most important we need to know in the various chemical reaction is the
rate of reaction.
The reaction occurred in a reactor is exothermic or endothermic. reactor is generally
assembled with a acket or coil in order to maintain the temperature in the reactor. 3f the heat
is evolved due to exothermic reaction+ a coolant stream is re&uired to pass through the acket
or coil to remove the extra heat. $n the other hand+ if endothermic reaction occurs in the
stream+ the flow of heating medium is passing through acket or coil for maintain the reaction
temperature. reactor operates at constant temperature+ then that is called as the isothermal
reactor. 3f any exothermic or endothermic reactions are involved in the reactor mixture varies
with time and we need to develop the energy balance e&uation for this non-isothermal reactor.
3n adiabatic reactor+ no interchange of heat occurs between the system and surroundings.
Thus no heating and cooling medium is re&uired. chemical reactor is a vessel where
reactions are carried out purposely to produce products from reactants by means of one or
chemical reactions. chemical reactor may be characteri4ed by the mode operation
according to the flow condition. 3n this experiment+ the Continuous Stirred Tank Reactor has
been used to conduct a chemical process.
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OBJECTIVES
• 5reparation of Calibration Curve for Conversion versus Conductivity
). To determine the conductivity at certain percent conversions.
,. To obtain a calibration curve of conductivity versus conversion.
• Effect of Residence Time on the Reaction in a CSTR
). To carry out the saponification reaction between #a$! and Et"c% in a CSTR.
,. To determine the effect of residence time+ τ on the extent of conversion.
/. To determine the reaction rate constant+ k.
THEORY
The continuous stirred-tank reactor "CSTR% or sometimes called back mix reactor was a very
typical reactor used in the industry as a part of the continuous-flow reactor. 6)+,+/7 The other
types of the continuous-flow reactor were plug-flow reactor "58R% and packed bed reactor
"52R%. 6,7 These reactors were classified as a continuous-flow reactor since the feed entered
the reactor continuously. The CSTR was named due to the special characteristic that it has
which is the stirrer as shown in the figure below. The function of the stirrer was to ensure allthe contents in well mixed condition and the concentration of the fluid was uniform
throughout the reaction.
Figure 1 The cross-sectional view of the CSTR
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The CSTR was generally designed to avoid the spatial variations in terms of the
concentrations+ temperature+ or even the reaction rate along the reaction process. Thus the
CSTR was operated in a steady state and it is normally used primarily for li&uid phase
reactions.6,7 3n such perfect mixing reaction+ the output composition was same to the material
inside the reactor where it is actually a function of residence time+ τ and rate of reaction+
−r .6/7 ll the variables such as the temperature and the concentration were the same at
every point either inside or at the exit of the reactor since the CSTR operated at steady state .6,7
The calculation performed by a CSTR was assumed as perfect mixing processes may be
initiated with the general mole balance e&uation+
F j0− F j+∫❑
V
r j dV =dN j
dt
Since the CSTR was operated at steady state+ thusdN j
dt =0 .6,+/7 This is due to no change
on the number of moles at steady state. *eanwhile+ the ∫❑
V
r j dV =V r j as there was no
spatial variations in the rate of reaction in a perfect mixing process. 6,7 Thus+ the general
mole balance became+
V = F j0− F j−r j
Theoretically+ the flow rate of a species was known as the product of the concentration of
species with the volumetric rate+
F j=C j×v
. 9hen inserting the flow rate e&uation into
the derived general mole balance+ 6,7
V =v0
C A 0−v C A−r A
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s for the effect of residence time on the percent of conversion in the CSTR+ the percent of
conversion should increase linearly as the time increase. 8or the experiment conducted+ the
residence time can be known based on the e&uationτ =
V CSTR
V 0.6)7
The e&uation used to find the conversion percent+ :+ 6)7
X =(1− C NaOH
C NaOH 0❑)×100
3n the experiment carried out+ in order to calculate the conversion percent+ the first thing that
should be determined was the volume of (.) * #a$! solution used to titrate '( ml of thesample collected from the CSTR. The sample solution initially being added with (.,' * !Cl
solution and three drops of phenolphthalein before conducting the titration process. The !Cl
was added for the &uenching purposes while the phenolphthalein was acted as an indicator.
The volume of the #a$! used was recorded as the colour of the sample changed from
colourless into light pink.
The calibration curve was also being carried out during this experiment by mixing the (.) *
of #a$! solution+ (.) * of Et"c% solution and also )(( ml of deionised water. The volume
for the #a$! solution and Et"c% solution were varied to achieve at certain percentage
conversion. The conductivity of all the solutions prepared based on their conversion were
then being observed by taking the value shown from a device called conductivity probe.
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APPARATUS AND MATERIALS
). The continuous-stirrer tank ;(0 "*$E0< 25);/%<
A. B. C. D. E.
F. G. H. I. J. K. L.
. Control 5anel =. Samples> *easuring Tank
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2. 8eed tanks "#a$! ? Et"c%% !. 5ipeline 9ith 8ittings
C. Stirrer 3. 9aste Tank
. *otor @. Aalves
E. Condenser B. Samples> ischarge 5ipe
8. 5umps 0. Tank Reactor
,. Retort stand with clamp./. '( ml burette.
;. '( ml+ )(( ml+ (( ml beakers
'. )( ml+ '( ml measuring cylinders
. ,'( ml conical flask
D. Sample of mixture<
a% '( ml sample solution
b% / drops of phenolphthalein
c% )( ml of (.,' * !Cl solution
. (.) * #a$! solution
F. (.) * Et"c% solution
)(. ropper )). Conductivity probe
),. eionised water
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PROCEDURE
A) GENERAL STARTUP PRCEDURE
). ll the following solutions are prepared<
a% ;( 0 of sodium hydroxide+ #a$! "(.)*%
b% ;( 0 of ethyl acetate+ Et"c% "(.)*%c% ) 0 of hydrochloric acid+ !C0 "(.,'*%+ for &uenching
,. ll valves are initially closed.
/. The feed vessels are charged as follows<
a% The charge port caps are opened for vessels 2) and 2,.
b% The #a$! solution are poured carefully into vessel 2) and the Et"c% solution
into vessel 2,.
c% The charge port caps are closed for both vessels.
;. The power for the control panel are turned on.'. Sufficient water in the thermostat T) tank are checked and refilled as necessary.
. Cooling water valve A)/ are opened and let the cooling water flow through the
condenser 9). "$nly for Experiment ,%
D. The overflow tube are adusted to give a working volume of )( 0 in the reactor R).
. Aalves A,+ A/+ AD+ A and A)) are all opened.
F. The unit is now ready for experiment.
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B) E!PERIMENTAL PROCEDURES
5reparation of Calibration Curve for Conversion vs. Conductivity
). ll the following solutions are prepared<
a% ) liter of sodium hydroxide+ #a$! "(.) *%
b% ) liter of sodium acetate+ Et"c% "(.) *%
c% ) liter of deionised water+ !,$
,. The conductivity and #a$! concentration for each conversion values are determined
by mixing the following solutions into )(( ml of deionised water<
a% (G conversion < )(( ml #a$!
b% ,'G conversion < D' ml #a$! H ,' ml Et"c%
c% '(G conversion < '( ml #a$! H '( ml Et"c%
d% D'G conversion < ,' ml #a$! H D' ml Et"c%e% )((G conversion < )(( ml Et"c%
C) BACK TITRATION PROCEDURES FOR MANUAL CONVERSION
DETERMINATION
). burette is filled up with (.) * #a$! solution.
,. )( ml of (.,' * !Cl is measured in a flask.
/. '( ml sample is obtained from the experiment and the sample is immediately added
to the !Cl in the flask to &uench the saponification reaction.
;. few drops of p! indicator is added into the mixture.
'. The mixture with #a$! solution is titrated from the burette until the mixture is
neutrali4ed. The amount of #a$! titrated is recorded.
D) EFFECT OF RESIDENCE TIME OF THE REACTION IN A CSTR
). The general start-up procedures are performed.
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,. 2oth pumps 5) and 5, are switched on simultaneously and valves A' and A)( are
opened to obtain the highest possible flow rate into the reactor.
/. 0et the reactor fill up with both the solution until it is ust about to overflow.
;. The valves A' and A)( are readusted to give a flow rate of about (.)( 01min. *ake
sure that both flow rates are the same. The flow rate are recorded.'. The stirrer *) is switched on and the speed are set to about ,(( rpm.
. The conductivity value at I3-;() is been monitored until it does not change over
time. This is to ensure that the reactor has reached steady state.
D. The steady state conductivity value is recorded and find the concentration of #a$! in
the reactor and extent of conversion from the calibration curve.
. Sampling valve A), is opened and collect a '( m0 sample. 2ack titration procedure
is carried out to manually determine the concentration of #a$! in the reactor and
extent of conversion.
F. The experiment "steps ' to F% are repeated for different residence times by adusting
the feed flow rates of #a$! and Et"c% to about (.)'+ (.,(+ (.,' and (./( 01min.
*ake sure that both flow rates are the same.
E) GENERAL SHUTDO"N PROCEDURE
). The cooling water valve A)/ is keep opened to allow the cooling water to continue
flowing.
,. 2oth pumps 5) and 5, are switched off. Stirrer *) is switched off.
/. The thermostat T) is switched off. 0et the li&uid in the reaction vessel R) cooled
down to room temperature.
;. Cooling water valve A)/ is closed.
'. Aalves A,+ A/+ AD and A are closed. Aalves A;+ AF and A), are opened to drain any
li&uid from the unit.
. The power for the control panel is turned off.
RESULT
A. PREPARATION OF CALIBRATION CURVE
Conversio
n
Solution *ixtures "0% Concentration of
#a$! "*%
Conductivity
"mS1cm%(.) * #a$! (.) * Et"c% !,$
(G (.) - (.) (.('(( );.;F(
,'G (.(D' (.(,' (.) (.(/D' .FF(
'(G (.(' (.(' (.) (.(,'( ;.D'(
D'G (.(,' (.(D' (.) (.(),' /.)'(
)((G - (.) (.) (.(((( (.),D
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Figure #$ =raph Conductivity against Conversion
B. E%%e&' (% Rei*e+&e Ti,e (% T-e Re&'i(+ i+ CSTR
• Reactor volume < ;( 0
• Concentration of #a$! in feed vessel < (.) *
• Concentration of Et"c% in feed vesssel < (.) *
Temperatu
re "oC%
8low
Rate
of
#a$!
"01mi
n%
8low
Rateof
Et"c
%
"01mi
n%
Total
8low
Rate of
Solution
s+ 8o
"01min%
Residen
ce Time+
J "min%
Conductivi
ty
Exit
Concentrati
on of
#a$!+ "*%
Conversio
n+ : "G%
,F. (.)( (.)( (.,( ,((.(( ,.; .; x )(-/ D.,
/(.( (.)' (.)' (./( )//.// ,., D.; x )(-/ '.,
/(., (.,( (.,( (.;( )((.(( ,.; . x )(-/
.(/(.; (.,' (.,' (.'( (.(( ,.D D.( x )(-/ D.,
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/(.' (./( (./( (.( .D ,.D) D.; x )(-/ '.,
Total 8low Rate of Solution+ 01min Aolume of #a$! titrated "m0%
(., ,).(./ ,)./
(.; ,).D
(.' ,).'
(. ,)./
Aolume of #a$!
titrated+A) "ml%
KAolume of unreacted
&uenching !Cl+ A, "ml%
Aolume of !Cl
reacted with #a$!
in sample+ A/ "ml%
*oles of !Cl
reacted with #a$!
in sample+n) "x)(-;%
,). .D, )., /.,(
,)./ .', ).; /.D(
,).D . )./, /./(
,).' .( ).;( /.'(
,)./ .', ).; /.D(
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CALCULATIONS
• Concentration of #a$! entering the reactor+ "C #a$!+o%<
C NaOH ,f
2
L
0.1 M
2
L (.(' *
• Aolume of unreacted &uenching !Cl+ "A,%<
C NaOH ,s
C HCl, s × V 1
L0.1 M
0.25 M x 21.8 mL
L .D, m0
• Aolume of !Cl reacted with #a$! in sample+ "A/%<
V HCl , s−V 2
L )( m0 M .D, m0
L )., m0
• *oles of !Cl reacted with #a$! in sample+ "n)%<
C NaOH , s× V 3
1000
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L0.25 M x1.28mL
1000
L /., x )(-;
• *oles of unreacted #a$! in sample+ "n,%
n2=n1 L /., x )(-;
• Concentration of unreacted #a$! in the reactor+ "C #a$!%<
n2
V s
1000
L3.2 x10−4
50×1000
L .; x )(-/ mol L
• Conversion of #a$! in the reactor+ :<
(1− C NaOH C NaOH , o )×100
L ") ‒6.4 x 10−3
0.05 ) x 100
= 87.2
• Reaction rate constant<
B L "C$- C%
CƬ ,
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= 0.05 ‒ (.; x )(-/%
,(( ‒ (.; x )(-/%,
L './,,/
-r L kC,
L ,.)(( x )(-;m
s
DISCUSSION
NOH / E'0A&) N0A&) / E'OH
The experiment was carried out by using special Sodium hydroxide "#a$!% and Ethyl
acetate and is conducted to carry out a saponification reaction between #a$! and Et"c% in
CSTR+ to carry out the manual conversion determination on experiment samples to verify the
conductivity measurement values of respective substances in the chemicals+ to determine the
effect of residence time onto the reaction extent of conversion and finally to determine the
reaction rate constant. 3n order to accomplish all of these obectives+ the Continuous Stirred
Tank Reactors "CSTR% ;(0 "model< 25 );/% is used. 2asically+ this experiment will mainly
be focusing on the saponification reaction of sodium hydroxide "#a$!% and Ethyl cetate+
Et"c%. Nsing the CSTR+ the behavior of the chemical reactors can be predicted+ therefore+
the key factors of a reactor such as the dimensions of the reactor+ can be estimated. The effect
of residence time onto the reaction extent of conversion and the reaction rate constant can be
determined after this experiment is carried out. 8or the titration part of the experiment+ it is to
determine the extent of conversion of the reaction using the manual conversion. fter all
these results are obtained+ both of these results will be compared.
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The saponification process+ which is one type of continuous process+ is a process to make
soap. 3n this experiment+ the reaction of saponification will involve &uenching with
hydrochloric acid to stop the reaction of neutrali4ation. The acid+ which is the Ethyl cetate+
Et"c% will be mixed with phenolphthalein in a beaker. The mixture will then be titrated with
Sodium !ydroxide in the burette. The titration process goes on until the mixture in the beaker
turns pink+ indicating the end point of the reaction that is the mixture has become neutral. The
reaction rate is very rapid+ and one must be very careful when reaching the end point of the
titration. $ther than that+ back titration is done to investigate the volume of Sodium
!ydroxide reacted.
3nside the reactor+ the saponification of #a$! and Ethyl cetate producing sodium acetate
and ethanol. $rder of the reaction is based on the powers of the concentration which areraised in the kinetic law. 8rom the data obtained+ a graph had been plotted which are
conductivity against conversion for manual conversion experiment "Titration% to determine
the conductivity of the reaction between #a$! and Et"c%. This graph should be plotted
before the beginning of the experiment so as to compare the results obtained later in the
experiment with the data shown in the calibration curve. 9ith the calibration curve+ one can
predict that conductivity of the reaction at any particular point in the reaction. 8rom =raph )+
it is observed that the conductivity will decrease when the volume of #a$! decreases.
Therefore+ it can be concluded that the conductivity decrease proportionately with
conversion+ :. This is because when volume of #a$! used decreases+ less #a$! will be
reacted with the acid in the titration. 9hen both reactants with different moles were used+ the
result will be different as this will give a significant difference in the conductivity of the
reaction. The product of the neutrali4ation are ethyl acetate and ethanol. 2ecause both of
these substances are not electric conductor and both Sodium ions and hydroxide ions ioni4e
easily in solution+ the conductivity of the mixture measurement depicts more or less+ the
concentration of #a$! that remains in the mixture. Therefore+ from the reading of
conductivity values of the mixture+ one can determine the concentration of unreacted #a$!
that remains in the solution relative to the conversion.
Aolumetric flow rate is related to the residence time therefore the experiment is repeated with
different flow rates+ that is (.)+ (.)'+ (.,(+ (.,' and (./( 01min. 8rom the data collected+ it
can be concluded that the conversion+ : increases as the volumetric flow rate decreases. The
fluid will enter the reactor at time+ t and will exit at time t H 2. Residence time+ 2 is the timethat the fluid elements spend in the reactor. t high flow rates+ the velocity of fluid moving in
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the reactor is high. This means the reactants spend less time within the reactor. 8rom the
second graph+ it can be observed that conversion+ : increases+ linearly with residence time.
Therefore+ it can be concluded that the longer the residence time+ the more conversion of the
reactant.
The reaction between #a$! and Et"c% is an e&uimolar reaction with the same initial
concentrations. 8rom the data obtained+ the order of the reaction was determined to be a
second order reaction. The rate law is Mr LkCC2. The rate of reaction is in 01mol.s. Relative
to the rate constant+ k for this order of reaction+ when the k value increases+ that means+ more
volume of #a$! is re&uired to convert one mole of #a$! in ) second. Calculated results
showed that the reaction rate constant increases as the volumetric flow rate decreases. 9hen
the reaction rate constant decreases+ the rate of reaction will increase. This is because thereare more moles of #a$! converted for a less volume of #a$! solution that is re&uired. This
is a very important fact to remember when designing a reactor so as to enable a reactor to
have a high conversion for large scale production. 2ased on result and the sample of
calculation+ the value of data was fitted to second order reaction. Therefore the rate law for
this experiments is<
*C3*' 4 5C#
The time taken for each sample taken is from the first minute the time started and followed
by the next 'th minute+ )(th minute and so on. The volume of titrating sodium hydroxide to
calculate the amount of &uenching hydrochloric acid+ phenolphtalein is used to be the
indicator of the mixture to be in neutral condition. Aolume of &uenching hydrochloric acid
unreacted with sodium hydroxide in sample is calculated using the amount of sodium
hydroxide titrated with the mixture.
The slopes of the graph are representing the specific reaction rate constant+ B. B constant can
be obtained by considering all the data obtained throughout the experiment. 2ased on the
calculation present on the sample of calculation+ B can be calculated.
8or the first temperature which is at ,F.OC+ since the reaction is second order+
-r L kC, L ,.)(( x )(-;
m
s . Then+ for this experiment+ the volume of &uenching !Cl
unreacted with #a$! in Sample "ml% is .D, ml. #ext+ the volume of !Cl reacted with
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#a$! in Sample "ml% is )., ml. The volume of titrating #a$! for this experiment are ,).
ml+ ,)./ ml+ ,).D ml+ ,).' ml+ and ,)./ ml.
This experiment also need to have the some precaution+ for example when if needed to read
the value of the sodium hydroxide from the burette+ make sure to look the value at eye level
to get the accurate value from the burette. The same person should be taking the reading since
everyone might have different opinion of the value.
CONCLUSION
s the result+ all of the aims and obectives are achieved. The reaction rate constant as well as
the effect of residence time on the conversion of Sodium !ydroxide has been determined.
8rom the result+ we obtained the order of the rate reaction which is second order.
Therefore
the reaction rate by the rate law is in the form of −r A=k C A2 and the result shows that the
conversion will decreases when the flow rate increases. This verifies the data and thus+ the
theory from the calibration curve from the first experiment. 9hen increasing the flow rate+
the reaction rate constant will be smaller and the rate of reaction will increase. The
experiment is has been achieved its obectives and successful.
RECOMMENDATION
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There are a few recommendations and precautions that have to be considered when
conducting this experiment in order to get accurate data and smoothly in progressing the
experiment. 8irstly+ general set-up must be conducted as given then followed by the
experimental procedures and end with the general shut-down procedures correctly. This is to
ensure that the experiment can be progress successfully. #ext is make sure reactor does not
have any leaks and valve closed and opened as needed. ll the valve must be controlled
carefully and slowly when adusting the flow rate to obtain (.)( 01min. 3t is to make sure
flow rate will stabili4e and the experiment will run smoothly and the result will be obtained
accurately. The titration process must be repeated for two or three times due to the errors
which is mostly came from the titration process. ll the apparatus that are been used in 2ack
Titration must be clean before proceed the next step and rinse after use it to make sure that it
will not affect the result. ue to saving the time used for finishing this experiment+ two
groups can be divided for conducting the CSTR while others carry out the back titration
process.
APPENDICES
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Figure 6$
Retort stand with burette which Figure 7$ *easuring cylinder
been used for back titration
Figure 8$ !ydrochloric acid "!Cl% Figure 9$ Sodium !ydroxide
"#a$!%
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