Reaction Kinetics ; Iodine Clock Reaction
Author
Michelle Vintimilla
Last Updated
7 years ago
License
Creative Commons CC BY 4.0
Abstract
The Hudson School, Hoboken, New Jersey. Chemistry, May 6th, 2015
The Hudson School, Hoboken, New Jersey. Chemistry, May 6th, 2015
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\title{
\normalfont \normalsize
\textsc{The Hudson School, Hoboken, New Jersey \\
Chemistry, May 6th,2015} \\
[10pt]
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\huge Reaction Kinetics ; Iodine Clock Reaction \\
\rule{\linewidth}{2pt} \\[10pt]
}
\author{Michelle Vintimilla}
\date{\normalsize \today}
\begin{document}
\maketitle
\noindent
Date Performed \dotfill May 6th,2015 \\
Partners \dotfill Kayla Eloi \\
Instructor \dotfill Ari Raisa \\
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\section{Purpose}
To find out the three things that affect the reaction rates. Those three things are catalysts, pressure, and concentration.
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\section{Hypothesis}
I hypothesize that both concentration and catalysts have an effect on reaction rates.
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\section {Materials}
\begin{itemize}\item
2 Graduated Cylinder (1000 mL)\end{itemize}
\begin{itemize}\item
Distilled Water\end{itemize}
\begin{itemize}\item
Tray\end{itemize}
\begin{itemize}\item
3 250 mL Beakers\end{itemize}
\begin{itemize}\item
3 400 mL Beakers\end{itemize}
\begin{itemize}\item
Stirring wand\end{itemize}
\begin{itemize}\item
Stopwatch\end{itemize}
\begin{itemize}\item
Thermometer\end{itemize}
\begin{itemize}\item
Hot Plate\end{itemize}
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\section {Procedure}
\begin{enumerate}\item Label 3 250 ml beakers 4a, 5a and 6a
Label 3 400 ml beakers 4b, 5b and 6b
\item In each of the b beakers put 10 mL of Na2S2O5, 30 mL of starch and 40 mL of water
\item In beakers 4a (45 C) and 5a (10 C) add 50 mL of KIO3 and 150 mL of Water
\item In Beaker 6a add 50 mL of KIO3, 140 mL of water and 10 mL (1 mL Acid, 9 mL water) H2SO4
\item Pour 4b into 4a quickly and start the timer the moment the liquids touch.
\item Stop when you see a color change. Repeat following the pattern with the remaining beakers.
\item Fill all the B beakers with the following:
.20 of Na2S2O5 (10 mL)
Starch (30mL)
H2O (40mL)
\item Fill 4A Beaker (45 Degrees C) with: 6 Seconds to convert
50 mL of KIO3
150 mL of H2O
\item Fill 5A (10 degrees C) with: 12 seconds to convert
50 mL of KIO3
150 mL of H2O
\item Fill 6A with (Room Temperature) : 3 seconds to convert
50 mL of KIO3
140 mL of H2O
10 ml of H2SO4 ( 1 mL of Acid, 9 mL of H2O)\end{enumerate}
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\section {Data}
\begin{table}[h]
\begin{tabular}{c c c c c c}
& \textbf{Beaker} & \textbf{Potassium Iodate (mL)} & \textbf{Distilled Water (mL)} & \textbf{Catalyst H2SO4} (mL) & \textbf{Temperature} \\
&1A &50 &150 &- &- \\
&2A &100 &100 &- &- \\
&3A &175 &25 &- &- \\
&4A &50 &150 &- &45 C \\
&5A &50 &150 &- &10 C \\
&6A &50 &149 &1 &- \\
\end{tabular}
\end{table}
\textbf{For all B beakers}
\begin{itemize}\item .20 of Na2S2O35 (10 mL)\end{itemize}
\begin{itemize}\item 30 mL of Starch\end{itemize}
\begin{itemize}\item 40 mL of H2O\end{itemize}
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\section {Discussion}
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\subsection{Definitions}
\begin{enumerate}\item \textbf{reaction kinetics:} a branch of chemistry that deals with the rate of chemical reactions, with factors influencing such rates, and with applications of rate studies to elucidate the mechanism of reactions.
\item\textbf{catalyst:} a substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change.
\item \textbf{concentration:} The amount of a substance per defined space. Concentration usually is expressed in terms of mass per unit volume.
\item \textbf{activation energy:} in chemistry, the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo chemical transformation or physical transport.\end{enumerate}
\subsection{Sources:}
\begin{itemize}\item http://www.merriam-webster.com/dictionary/reaction%20kinetics
\item http://dictionary.reference.com/browse/catalyst
\item http://chemistry.about.com/od/chemistryglossary/g/concentration.htm
\item http://www.britannica.com/EBchecked/topic/4535/activation-energy
\item http://www.explainthatstuff.com/catalyticconverters.html
\item http://chemwiki.ucdavis.edu \end{itemize}
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\subsection{Results}
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Beaker 4a: 6 seconds
Beaker 5a: 12 seconds
Beaker 6a: 3 seconds
\subsection{Questions}
\begin{enumerate}\item What could be a good synonym for reaction kinetics?
\textbf{Chemical Kinetics}
\item Which reaction was the reference reaction? What does that mean?
\item What were the three variables that had an effect on reaction rates?
\textbf{Catalysts, concentration and temperature}
\item How does the collision model of chemical reactions explain reaction rates?
\textbf{A chemical reaction occurs only when reactant molecules,ions, or atoms collide with an excess amount of kinetic energy and in "the proper orientation." The collision model explains why most collisions between molecules do not result in a chemical reaction (for example).}
\item What are catalysts called in living organisms?
\textbf{Enzymes}
\item What kind of catalysts do cars have? Hint: look up catalytic converters
\
\textbf{Catalytic converters are also known as Cats/Cat-cons. They aid in converting harmful chemicals in vehicles exhausts into gases that are harmless, such as steam.}
\item How do catalysts work?
\textbf{
A catalyst works by providing an alternative reaction pathway to the reaction product. The rate of the reaction is increased as this alternative route has a lower activation energy than the reaction route not mediated by the catalyst.
A catalyst works by providing a convenient surface that enables a different route for a chemical reaction to occur.The reacting particles on the catalyst surface collide more frequently with each other and more of the collisions result in a chemical reaction because the different route provided by the catalyst has a lower activation energy.}
\item What is the actual reaction equation for this iodine clock reaction?
\includegraphics[width=12cm, height=5cm]{FullSizeRender__3_.jpg} \end{enumerate}
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\subsection{Critique}
Explain the difficulties in the method for timing (assuming that all solutions were prepared correctly) and suggest improvements.
\textbf{Never use beaker to measure volume, use a graduated cylinder. }
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\section{Conclusion}
Our hypothesis was right. Both the concentration and the catalyst had an affect on the reaction rates causing each reactions to either increase or decrease in time. From doing this lab I learned
\begin{enumerate}\item How to efficiently use Overleaf to create a lab. \end{enumerate}
\begin{enumerate}\item The factors that affect reaction rates. \end{enumerate}
\begin{enumerate}\item \end{enumerate}
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