Kinetics I Lab Report (1)

Kinetics I Lab Report The Rate Equation between Oxalic Acid and Potassium Permanganate Permanganate Purpose: Kinetics is defned as the measurement o rates o reactions! In order to "alidate the importance o concentration on the rates o reactions# we experimentall$ manipulated the molarit$ o oxalic acid and potassium permanganate to determine the o"erall rate o reaction between them! In the lab# the time the reaction ta%es to ull$ occur was mar%ed b$ a color change called colorimetric anal$sis! The equipment used include "olumetric glassware# test tubes# stirring rods# and a pipet! Procedure: &ollowed the experimental procedure as per the laborator$ manual! 'ariations 'ariations made to the procedure include not utili(ing the Eriochrome )lac% T tube and instead stopping the timer when the solution solutio n transitioned to the color $ellow $ello w! Data:

Table *+ ,ata or Experiment -* .onditions T/01!12°. T r ia l 3K4nO56 370.0O56 Time 8s9 * 0 1

!2*2; !2*2; !2*2;

A"erage Rate+ >!**x*2?< 4: 4:s ?@ .onfdence λ+ 5!;5x*2

!1*< !1*< !1*<

*5= ! 5 *<> ! > *<* ! @

tandard ,e"iation+ *!=
Table 0+ ,ata or Experiment -0 .onditions T/01!;=°. T r ia l 3K4nO56 370.0O56 Time 8s9 * 0 1

!2*2; !2*2; !2*2;

A"erage Rate+ *!*=x*2?5 4: 4:s ?< .onfdence λ+ 0!05x*2

!@0= !@0= !@0=

;5!@ =*!* =;!5

tandard ,e"iation+ =!22x*2?@ 4: 4:s

Table 1+ ,ata or Experiment -1 .onditions T/01!;=°. T r ia l 3KmnO56 370.0O56 Time 8s9 * 0 1

!20*> !20*> !20*>

A"erage Rate+ *!1;x*2?5 4: 4:s ?< .onfdence λ+ 0!**x*2

!1*< !1*< !1*<

*<> ! > *@; ! 2 *5; ! 1

tandard ,e"iation+ ;!<2x*2?@ 4: 4:s

Reaction Order Data:

Reaction Order C 8rounded to nearest tenth9+ *!2

Rate*/3K4nO56: time >!01x*2?< @!;!*0x*2?< =
Rate*/3KmnO56: time *!0;x*2?5 *!*=x*2?5 *!*2x*2?5 =
Rate*/3KmnO56: time *!1;x*2?5 *!0=x*2?5 *!5@x*2?5 =
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Reaction Order D 8rounded to nearest tenth9+ 2!> O"erall Order o Reaction CD+ CD+ %3K4nO 56*!2370.0O562!> 8*!22!>/*!>9 Rate .onstant# %+ !2*< L:mFs cons tant Results and Conclusions: The goal o this lab was to determine the rate constant through "arious sets o reactions between potassium permanganate and oxalic acid! It was disco"ered throughout the conduction o this experiment that reactions that contain diGerent concentrations o the same solution will react "er$ diGerentl$# diGerentl$# and the time or the reaction to occur could happen in a "er$ wide arra$ o times! The use o potassium permanganate and oxalic acid were helpul when determining the rate constant because the experimenters could obser"e the color change o the solution# which can get a close:accurate result on the time that was ta%en or the reaction to occur! occur! The experimenters perormed multiple mul tiple trials 819 o the same experiment# so thereor the a"erage rate o the reaction could be used# which is more accurate than Hust using the "alue rom one trial! The technique perormed was "er$ successul! This can be supported b$ the similarit$ in reaction times or each trial in an experiment! The closeness in these "alues as well as the rate shows that the perormance o the experiment was done so successull$ and consistentl$! consistentl$! Also# the standard de"iation "alues show good accurac$! accurac$! In regards to the rate constant# the "alue seems to be accurate because it is within the same range as some o the other experimenters "alues who perormed the same experiment! The data that was gathered during and ater the conduction o this experiment was "alid! Each trial o o  each experiment was close in range to the other# which shows precision! It was shown in this experiment that the solution with the most oxalic acid# had the largest reaction rate! It was expected beore the conduction o this experiment that all o the rates would be in a "er$ close range to each other# other# mainl$ because the total "olumes or all the experiments remained constant# as well as the chemical reagents used! Ater the experiment howe"er# howe"er# it was ound that diGerent molarities and "olumes added into a solution can highl$ "ar$ and alter the time in which the experiment will react! A maHor part o this lab was fnding the reaction order C and D# D# as well as the rate constant or this specifc s pecifc reaction! To fnd reaction order C and D# D# a ormula was used using the a"erage rates rom experiment one and three# as well as the molarit$ concentration o potassium permanganate! These "alues were then reerred to as x and $# $# and were then used to determine the rate constant! To To fnd this "alue# the molarit$ molar it$ concentration o potassium permanganate as well as oxalic acid were raised rais ed to the power o x and $# $# which were Hust ound in the pre"ious step# and was set equal to the a"erage rate o experiment o experiment one! The o"erall order o reaction re action was ound b$ Hust adding the "alues o x and $! $! The possible errors that could ha"e occurred while perorming this experiment include adding too much or too little o a certain solution to a test tube! This could drasticall$ alter the "alues o the rate constant and would thereor throw oG all o the data ound throughout the entire experiment! Another error could ha"e been not stirring the mixture long enough# so the reaction ne"er ull$ occurred! The time "alues would then be oG# which would thereore alter "alues such as the a"erage rate and the rate constant! Also# the stirring could ha"e changed the results# because during one trial#



disco"ered that the reaction times and the reaction rate could Juctuate greatl$# greatl$# depending on the concentration o specifc solutions! It was also learned the colorimetric anal$sis is a "er$ simple and eGecti"e wa$ to determine the rate law o the reaction between potassium permanganate and oxalic acid! Although there is room or error when basing an experiment and reaction oG color change# multiple trials help to buGer the room or error that ma$ exist! 7owe"er# 7owe"er# it is quite simple s imple to obtain the rate constant and other "alues such as the reaction re action orders with use o an experiment and ormulas! In conclusion# or this particular experiment# the higher the concentration o oxalic acid# the higher the a"erage rate reaction time! 7igh a"erage rates could be caused b$ man$ diGerent solutions that are part o other mixtures! This lab was an eGecti"e wa$ to connect the idea o reaction to a constant that is used in science consistentl$ the rate constant! Sample Calculations/Questions: Calculations/Questions: ee attached sheet!

Kinetics I Lab Report (1)

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