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% Document Info
\author{anupamabalaji}
\pdfinfo{
  /Title (ial-chem-unit-4-kinetics.pdf)
  /Creator (Cheatography)
  /Author (anupamabalaji)
  /Subject (IAL Chem Unit 4 Kinetics Cheat Sheet)
}

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\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{IAL Chem Unit 4 Kinetics Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{anupamabalaji} via \textcolor{DarkBackground}{\uline{cheatography.com/213395/cs/46424/}}}
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\noindent
\begin{multicols}{3}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}anupamabalaji \\
  \uline{cheatography.com/anupamabalaji} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 22nd May, 2025.\\
   Updated 22nd May, 2025.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{x{3.04 cm} x{4.96 cm} }
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Key Definitions}}  \tn
% Row 0
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{\bf{Term}} & {\bf{Definition}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Rate of Reaction & Change in concentration of a reactant or product per unit time. \tn 
% Row Count 4 (+ 3)
% Row 2
\SetRowColor{LightBackground}
Rate Equation & Rate = {\emph{k}} {[}A{]}\textasciicircum{}m\textasciicircum{} {[}B{]}\textasciicircum{}n\textasciicircum{} where m, n are the orders of the reaction. \tn 
% Row Count 7 (+ 3)
% Row 3
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Order of Reaction & The power to which the concentration of a reactant is raised in the rate law \tn 
% Row Count 11 (+ 4)
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Overall Order & The sum of the powers (orders) of all reactants in the rate equation. Order = m+n. \tn 
% Row Count 15 (+ 4)
% Row 5
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Half-life (t\textasciitilde{}₁⁄₂\textasciitilde{}) & Time taken for the concentration of a reactant to fall to half its value. \tn 
% Row Count 19 (+ 4)
% Row 6
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Rate Constant (k) & Proportionality constant in the rate equation; depends on temperature. \tn 
% Row Count 22 (+ 3)
% Row 7
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Activation Energy (Eₐ) & Minimum energy needed for a reaction to occur. \tn 
% Row Count 24 (+ 2)
% Row 8
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Adsorption & The binding of molecules to a surface (such as a catalyst), which increases reaction rate. \tn 
% Row Count 28 (+ 4)
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Desorption & The release of products from a catalyst surface after the reaction. \tn 
% Row Count 31 (+ 3)
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\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Arrhenius Equation}}  \tn
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\mymulticolumn{1}{x{8.4cm}}{k=Ae\textasciicircum{}E\textasciitilde{}a\textasciitilde{}/RT\textasciicircum{} \newline Where \newline k = Chemical Reaction Rate \newline A = Pre-exponential factor \newline E\textasciitilde{}a\textasciitilde{} = Activation Energy \newline R = Gas Constant \newline T = Temperature in Kelvin}  \tn 
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\mymulticolumn{3}{x{8.4cm}}{\bf\textcolor{white}{Mechanisms: SN1 vs SN2}}  \tn
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{\bf{Feature}} & {\bf{SN1}} & {\bf{SN2}} \tn 
% Row Count 2 (+ 2)
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Steps & 2 steps (carbocation formed) & 1 step (simultaneous attack/leave) \tn 
% Row Count 5 (+ 3)
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\seqsplit{Reactivity} & Tertiary haloalkanes & Primary haloalkanes \tn 
% Row Count 7 (+ 2)
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Rate Law & rate = k{[}haloalkane{]} & rate = k{[}haloalkane{]}{[}Nu⁻{]} \tn 
% Row Count 9 (+ 2)
% Row 4
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Steric \seqsplit{Hindrance} & Low (carbocation intermediate) & High (due to nucleophile approach) \tn 
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\mymulticolumn{3}{x{8.4cm}}{\bf\textcolor{white}{Experimental Techniques}}  \tn
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{\bf{Method}} & {\bf{Measurement}} & {\bf{Used For}} \tn 
% Row Count 2 (+ 2)
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Mass loss & Decreasing mass (gas released) & Rate of gas-producing reactions \tn 
% Row Count 4 (+ 2)
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\seqsplit{Volume} of gas & Gas syringe / upside-down cylinder & Gas evolution \tn 
% Row Count 7 (+ 3)
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\seqsplit{Titration} & Concentration vs time & Accurate kinetic data \tn 
% Row Count 9 (+ 2)
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\seqsplit{Colorimetry} & Absorbance vs concentration & Colored species (e.g. I₂ reaction) \tn 
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{\bf{Order}} & {\bf{Rate Law}} & {\bf{Half-life}} \tn 
% Row Count 2 (+ 2)
% Row 1
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Zero & rate = k & t\textasciitilde{}₁⁄₂\textasciitilde{} = {[}A{]}₀ / 2k \tn 
% Row Count 4 (+ 2)
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First & rate = k{[}A{]} & t\textasciitilde{}₁⁄₂\textasciitilde{} = ln2 / k \tn 
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Second & rate = k{[}A{]}$^{\textrm{2}}$ & t\textasciitilde{}₁⁄₂\textasciitilde{} = 1 / (k{[}A{]}₀) \tn 
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\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Rate Determining Step (RDS)}}  \tn
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\mymulticolumn{1}{x{8.4cm}}{1. The slowest step in a mechanism controls the overall rate. \newline % Row Count 2 (+ 2)
2. Only species involved up to RDS appear in the rate equation. \newline % Row Count 4 (+ 2)
3. Powers in rate law = number of molecules in RDS.% Row Count 6 (+ 2)
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{\bf{Type}} & {\bf{Phase}} & {\bf{Example}} & {\bf{Notes}} \tn 
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\seqsplit{Homogeneous} & Same as \seqsplit{reactants} & Fe$^{\textrm{2}}$⁺/Fe$^{\textrm{3}}$⁺ in S₂O₈$^{\textrm{2}}$⁻ + I⁻ & Catalyst regenerated via redox steps \tn 
% Row Count 5 (+ 3)
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\seqsplit{Heterogeneous} & \seqsplit{Different} from \seqsplit{reactants} & Fe in Haber process & Provides surface, weakens bonds, speeds reaction \tn 
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\mymulticolumn{4}{x{8.4cm}}{Catalysts lower the activation energy of a reaction by providing an alternate reaction route.}  \tn 
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\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Adsorption (in Heterogeneous Catalysis)}}  \tn
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\mymulticolumn{1}{x{8.4cm}}{Adsorption is when reactant molecules bind to active sites on the surface of a solid catalyst. \newline  \newline This: \newline 1. Brings molecules close together, increasing collision frequency \newline 2. Weakens bonds in the reactants, lowering activation energy \newline 3. Allows for a faster reaction \newline  \newline After the reaction, products desorb (leave) from the surface, freeing the site for reuse.}  \tn 
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% That's all folks
\end{multicols*}

\end{document}