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\author{NescafeAbusive32 (nescafeabusive32)}
\pdfinfo{
  /Title (gr-12-energy-changes-and-rates-of-reaction.pdf)
  /Creator (Cheatography)
  /Author (NescafeAbusive32 (nescafeabusive32))
  /Subject (Gr. 12 Energy Changes and Rates of Reaction Cheat Sheet)
}

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    {\parbox{\dimexpr\textwidth-2\fboxsep\relax}{\noindent
        \hspace*{-6pt}\includegraphics[width=5.8cm]{/web/www.cheatography.com/public/images/cheatography_logo.pdf}}
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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Gr. 12 Energy Changes and Rates of Reaction Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{NescafeAbusive32 (nescafeabusive32)} via \textcolor{DarkBackground}{\uline{cheatography.com/53385/cs/14452/}}}
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\noindent
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}NescafeAbusive32 (nescafeabusive32) \\
  \uline{cheatography.com/nescafeabusive32} \\
  \end{tabulary}
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 24th January, 2018.\\
   Updated 24th January, 2018.\\
   Page {\thepage} of \pageref{LastPage}.
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Sponsor}}  \\
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  \vspace{-5pt}
  %\includegraphics[width=48px,height=48px]{dave.jpeg}
  Measure your website readability!\\
  www.readability-score.com
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\begin{document}
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\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{x{2.23965 cm} x{2.73735 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Introduction}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Thermochemistry:}} the study of the {\bf{energy changes}} that accompany physical or chemical changes in matter} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Types of energy:}}} \tn 
% Row Count 4 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\{\{bt\}\}{\bf{E`p}}` (potential energy) & \{\{bt\}\}the energy of an object due to its {\bf{position/composition}} \tn 
% Row Count 7 (+ 3)
% Row 3
\SetRowColor{white}
\{\{bb\}\}{\bf{E`k`}} (kinetic energy) & \{\{bb\}\}the energy of an object due to its {\bf{motion}} \tn 
% Row Count 10 (+ 3)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Thermal energy}} (E`th`): the {\bf{total quantity}} of {\bf{E`k` and E`p`}} in a substance; depends on how fast the particles are moving: more energy = more speed = more E`th`} \tn 
% Row Count 14 (+ 4)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Heat:}} the transfer of E`th` {\bf{from a warm object to a cool object}}} \tn 
% Row Count 16 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Temperature:}} measure of the {\bf{average E`k`}} of the particles in a substance} \tn 
% Row Count 18 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Law of Conservation of Energy:}} energy {\bf{cannot be created or destroyed}}, only converted from one form to another} \tn 
% Row Count 21 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{{\emph{Note:}}}} Temperature ≠ E`th`! A cup of water at 90°C has a higher temperature than a bathtub of water at 40°C, but the water has more E`th` since it has more molecules}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{1.69218 cm} x{3.28482 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{System/Surroundings and Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{System:}} the group of {\bf{reactants and products}} being studied} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bb\}\}{\emph{Surroundings:}} all the matter that is {\bf{not}} a part of the system} \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bb\}\}{\bf{Types of systems:}}} \tn 
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% Row 3
\SetRowColor{white}
{\bf{Open system}} & both energy and matter are allowed to enter and leave freely \tn 
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% Row 4
\SetRowColor{LightBackground}
{\bf{Closed system}} & energy can enter and leave the system, but matter cannot \tn 
% Row Count 11 (+ 3)
% Row 5
\SetRowColor{white}
{\bf{Isolated system}} & neither matter are allowed to leave the system (complete isolation is {\bf{impossible}}) \tn 
% Row Count 15 (+ 4)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Types of reactions:}}} \tn 
% Row Count 16 (+ 1)
% Row 7
\SetRowColor{white}
\{\{bt\}\}{\bf{Endothermic}} & \{\{bt\}\}energy from the surroundings is {\bf{absorbed}} by the system \tn 
% Row Count 19 (+ 3)
% Row 8
\SetRowColor{LightBackground}
{\bf{Exothermic}} & energy from the system is {\bf{released}} into the surroundings \tn 
% Row Count 22 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{1.9908 cm} x{2.9862 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Specific Heat Capacity and Calorimetry}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Specific heat capacity:}} the amount of energy required to {\bf{raise the temperature}} of 1 g of a substance {\bf{by 1°C}} (measured in J/g°C); depends on {\bf{type}} and {\bf{form}} of substance} \tn 
% Row Count 4 (+ 4)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Calorimetry:}} the experimental process of measuring the {\bf{ΔE`th`}} in a {\bf{chemical or physical}} change} \tn 
% Row Count 7 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bb\}\}{\emph{Calorimeter:}} device used to {\bf{measure ΔE`th`}}} \tn 
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% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bb\}\}{\bf{Types of calorimeters:}}} \tn 
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% Row 4
\SetRowColor{LightBackground}
{\bf{Polystyrene}} (styrofoam) & Reasonably accurate and inexpensive \tn 
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% Row 5
\SetRowColor{white}
{\bf{Bomb}} & More precise, used for reactions that involve gases \tn 
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% Row 6
\SetRowColor{LightBackground}
{\bf{Flame}} & Used for combustion reactions \tn 
% Row Count 17 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Calorimetry Calculations}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{4 assumptions when performing calorimetry calculations:}}} \tn 
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% Row 1
\SetRowColor{white}
1. Any thermal energy transferred from the calorimeter to the outside environment is negligible & 3. All dilute, aqueous solutions have the same density as water (D = 1.00 g/mL) \tn 
% Row Count 7 (+ 5)
% Row 2
\SetRowColor{LightBackground}
2. Any thermal energy absorbed by the calorimeter itself is negligible & 4. All dilute, aqueous solutions have the same specific heat capacity as water (c = 4.18 J/g°C) \tn 
% Row Count 12 (+ 5)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Calorimetry formula:}}} \tn 
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% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{Q = mcΔT}}} \tn 
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% Row 5
\SetRowColor{white}
{\bf{m =}} mass of the substance (g) & {\bf{c =}} specific heat capacity of the substance ( J/g°C) \tn 
% Row Count 17 (+ 3)
% Row 6
\SetRowColor{LightBackground}
{\bf{ΔT =}} temperature change experienced by the system; ΔT = T`final` - T`initial` (°C) & {\bf{Q =}} total amount of E`th` absorbed/released by a chemical system ( J ) \tn 
% Row Count 22 (+ 5)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Value of {\bf{Q}} has two parts: \newline The {\bf{number}}: how much energy is involved \newline The {\bf{sign}}: the direction of the energy transfer (important to show, {\bf{even if it is positive!}}) \newline  \newline Because of the law of conservation of energy, the total thermal energy of the system and the surroundings remain constant: \newline  \newline {\bf{Q`system` + Q`surroundings` = 0}} \newline {\bf{Q`system` = - Q`surroundings`}}}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Enthalpy Change (ΔH)}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Enthalpy}} (H): the total amount of E`th` in a system; {\bf{not directly measurable}}} \tn 
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% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Must measure {\bf{enthalpy change (ΔH)}} by measuring the {\bf{ΔT}} in the {\bf{surroundings}}} \tn 
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% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Enthalpy change}} (ΔH): the energy {\bf{released to/absorbed from the surroundings}} during a chemical/physical change; can be measured {\bf{using calorimetry data}}} \tn 
% Row Count 8 (+ 4)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{As long as pressure is constant, the enthalpy change of a chemical system is equal to the {\bf{flow of thermal energy in or out of the system}}} \tn 
% Row Count 11 (+ 3)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Enthalpy change formula:}}} \tn 
% Row Count 12 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{ΔH = |Q`system`|}}} \tn 
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% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{ΔH = ±|Q`surroundings`|}}} \tn 
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% Row 7
\SetRowColor{white}
If ΔH \textgreater{} 0, the reaction is {\bf{endothermic}} & If ΔH \textless{} 0, the reaction is {\bf{exothermic}} \tn 
% Row Count 17 (+ 3)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{If there is {\bf{more than one substance}} making up the surroundings (i.e. {\bf{bomb/flame calorimeters}}), then} \tn 
% Row Count 20 (+ 3)
% Row 9
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{Q`surroundings` = Σ Q`substances`}}} \tn 
% Row Count 21 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Molar Enthalpy Change (ΔH`x`)}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Molar enthalpy change}} (ΔH`x`): the enthalpy change {\bf{associated with}} a physical/chemical change involving {\bf{1 mol of a substance}} (J/mol)} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{{\emph{x}} = type of change}} (vaporization, neutralization, combustion, etc.)} \tn 
% Row Count 5 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Molar enthalpy change formula:}}} \tn 
% Row Count 6 (+ 1)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{ac\}\}{\bf{ΔH = nΔH`x`}}} \tn 
% Row Count 7 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Representing Enthalpy Change}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{4 ways to represent ΔH:}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
1. Thermochemical equations with {\bf{energy terms}} & CH`4` + 2 O`2` \{\{fa-long-arrow-right\}\} CO`2` + 2 H`2`O + {\bf{890.8 kJ}} \tn 
% Row Count 5 (+ 4)
% Row 2
\SetRowColor{LightBackground}
2. Thermochemical equations with {\bf{ΔH terms}} & CH`4` + 2 O`2` \{\{fa-long-arrow-right\}\} CO`2` + 2 H`2`O  {\bf{ΔH = -890.8 kJ}} \tn 
% Row Count 9 (+ 4)
% Row 3
\SetRowColor{white}
3. Molar enthalpies {\bf{(ΔH`x`)}} & ΔH`comb` = -890.8 kJ/mol \tn 
% Row Count 11 (+ 2)
% Row 4
\SetRowColor{LightBackground}
4. Potential energy {\bf{(E`p`)}} diagrams & \{\{popup="http://www.swotrevision.com/pages/alevel/chemistry/images/img\_64.GIF"\}\}See an example here\{\{/popup\}\} \tn 
% Row Count 17 (+ 6)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Hess' Law}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Enthalpy change (ΔH) is determined by {\bf{initial and final conditions}} of a system; it is {\bf{independent}} of the pathway} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{The total ΔH of a multi-step reaction is the {\bf{sum of the ΔH}} of its {\bf{individual steps}}} \tn 
% Row Count 5 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Hess's Law formula:}}} \tn 
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% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{ΔH`reaction` = Σ ΔH`steps`}}} \tn 
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% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{This formula can be used in cases where the {\bf{overall reaction is not feasible to be done in a calorimeter}} (i.e. reaction is too slow/too fast/too violent)} \tn 
% Row Count 11 (+ 4)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Rules:}}} \tn 
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% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{1. If a reaction is {\bf{flipped}}, flip the ΔH value's sign} \tn 
% Row Count 14 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{2. If a reaction is {\bf{multiplied}}, multiply the ΔH value} \tn 
% Row Count 16 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Standard Enthalpy of Formation (ΔH°`f`)}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{The standardized ΔH when {\bf{1 mol}} of a substance is formed ({\bf{synthesized}}) directly from its elements to its {\bf{standard state at SATP}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{The elements themselves have a ΔH°`f` of {\bf{0}} (elements {\bf{cannot be synthesized}})} \tn 
% Row Count 5 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Bond Energies (D) and Bond Enthalpy}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bb\}\}{\bf{Bond Energies}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Stability of a molecule is related to the {\bf{strength of its covalent bonds}}} \tn 
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% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{The {\bf{strength}} is determined by the {\bf{energy required to break that bond}}} \tn 
% Row Count 5 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Bond Enthalpy:}}} \tn 
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% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}ΔH for breaking a particular bond in {\bf{1 mol of a gaseous substance}}} \tn 
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% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Always positive}} because energy is always required to break bonds} \tn 
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% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Used for {\bf{predicting reaction types}} before the reaction is performed ({\bf{not entirely accurate}})} \tn 
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% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Formula for predicting reaction type using D and bond H:}}} \tn 
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% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{ΔH = Σ (nD`bonds broken`) - Σ (nD`bonds formed`)}}} \tn 
% Row Count 16 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{3.43413 cm} x{1.54287 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Reaction Rates}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{The {\bf{speed}} at which a reaction {\bf{occurs}}} \tn 
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% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Can be {\bf{fast}} (10\textasciicircum{}-15\textasciicircum{}s) or {\bf{slow}} (years)} \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Measured by the {\bf{change}} in the amount of {\bf{reactants consumed}} or {\bf{products formed}} at a given time interval(s)} \tn 
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% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Can be measured by {\bf{volume}}, {\bf{mass}}, {\bf{colour}}, {\bf{pH}}, and {\bf{electrical conductivity}}} \tn 
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% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Often expressed as a {\bf{positive value}} for convenience, regardless of what is being measured} \tn 
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% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Average rate of reaction:}} rate of a chemical reaction {\bf{between two points in time}} (one time interval); calculated from the {\bf{slope of the secant}} of the time interval on a {\bf{concentration-time graph}}} \tn 
% Row Count 14 (+ 5)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Average rate of reaction formulas:}}} \tn 
% Row Count 15 (+ 1)
% Row 7
\SetRowColor{white}
How fast a {\bf{reactant disappears}} & \textasciicircum{}- Δ{[}A{]}\textasciicircum{}/`Δt` \tn 
% Row Count 17 (+ 2)
% Row 8
\SetRowColor{LightBackground}
How fast a {\bf{product appears}} & \textasciicircum{}Δ{[}B{]}\textasciicircum{}/`Δt` \tn 
% Row Count 19 (+ 2)
% Row 9
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Δ{[}A{]}}}, {\bf{Δ{[}B{]}}}, {\bf{{\emph{Δt}}}} = {\emph{{[}A{]}`2` - {[}A{]}`1`}}, {\bf{{[}B{]}`2` - {[}B{]}`1`}}, {\bf{{\emph{t`2` - t`1`}}}}} \tn 
% Row Count 21 (+ 2)
% Row 10
\SetRowColor{LightBackground}
\{\{bt\}\}Units & \{\{bt\}\}mol/L⋅s \tn 
% Row Count 23 (+ 2)
% Row 11
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Instantaneous rate of reaction:}} rate of a chemical reaction at a {\bf{single point int time}}; calculated from the {\bf{slope of the tangent}} of the time position on a {\bf{concentration-time graph}}} \tn 
% Row Count 28 (+ 5)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Collision Theory}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{States that chemical reactions can only occur if the reactants have the right {\bf{kinetic energy (speed)}} and {\bf{orientation}} to break reactant bonds and form product bonds} \tn 
% Row Count 4 (+ 4)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Effective collision:}} a collision that has {\bf{sufficient energy}} and {\bf{correct orientation}} of colliding particles to {\bf{start a reaction}}} \tn 
% Row Count 7 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Ineffective collision:}} a collision where the particles rebound, {\bf{unchanged in nature}}} \tn 
% Row Count 9 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Activation energy}} (E`a`): the {\bf{minimum energy required}} for reactants to have for a collision to be effective} \tn 
% Row Count 12 (+ 3)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Activated complex/transition state:}} {\bf{unstable arrangement of atoms}} containing {\bf{partially formed}} and {\bf{partially broken bonds}}; {\bf{maximum E`p` point}} in the reaction} \tn 
% Row Count 16 (+ 4)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Rate of a reaction depends on the {\bf{frequency of collisions}} and the {\bf{fraction of those collisions}} that are {\bf{effective}}.\{\{bt\}\}} \tn 
% Row Count 19 (+ 3)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\} Rate = {\bf{frequency}} of collisions x {\bf{fraction of collisions}} that are {\bf{effective}}} \tn 
% Row Count 21 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Increasing Reaction Rates}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{5 factors that can increase a reaction rate: {\bf{chemical nature}} of reactants, {\bf{concentration}}, {\bf{surface area}}, {\bf{temperature}}, and {\bf{catalysts}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Chemical nature of reactants}}} \tn 
% Row Count 4 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}For any reactant, the activation energy required depends on the {\bf{bond type}} (single vs double vs triple), the {\bf{bond strength}} ({\emph{D}} value), the {\bf{number of bonds}}, and the {\bf{size and shape}} of the molecule(s)} \tn 
% Row Count 9 (+ 5)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Concentration of reactants}}} \tn 
% Row Count 10 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\emph{Concentration}} = amount of substance per unit volume (mol/L); applies only to {\bf{solutions}}} \tn 
% Row Count 12 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{fa-long-arrow-up\}\}{[}reactant{]} = \{\{fa-long-arrow-up\}\}collisions = \{\{fa-long-arrow-up\}\}rate} \tn 
% Row Count 14 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Rate α {[}reactant{]}}} - as the {\bf{concentration increases}}, the {\bf{rate increases}}, and vice versa} \tn 
% Row Count 16 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Surface area}}} \tn 
% Row Count 17 (+ 1)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\emph{Surface area}} = total area of all the surfaces of a {\bf{solid}} figure} \tn 
% Row Count 19 (+ 2)
% Row 9
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{fa-long-arrow-up\}\}SA = \{\{fa-long-arrow-up\}\}collisions = \{\{fa-long-arrow-up\}\}rate} \tn 
% Row Count 21 (+ 2)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Rate α SA}} - as the {\bf{surface area increases}}, the {\bf{rate increases}}, and vice versa} \tn 
% Row Count 23 (+ 2)
% Row 11
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Temperature of system}}} \tn 
% Row Count 24 (+ 1)
% Row 12
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}\{\{fa-long-arrow-up\}\}T = \{\{fa-long-arrow-up\}\}collisions + \{\{fa-long-arrow-up\}\}fraction of effective collisions = \{\{fa-long-arrow-up\}\}rate} \tn 
% Row Count 27 (+ 3)
% Row 13
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Rate α T}} - as the {\bf{temperature increases}}, the {\bf{rate increases}}, and vice versa} \tn 
% Row Count 29 (+ 2)
% Row 14
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Catalyst}}} \tn 
% Row Count 30 (+ 1)
\end{tabularx}
\par\addvspace{1.3em}

\vfill
\columnbreak
\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Increasing Reaction Rates (cont)}}  \tn
% Row 15
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\emph{Catalyst}} = substance that {\bf{increases the rate}} of a reaction {\bf{without itself being consumed}} in the reaction; provide an {\bf{alternate pathway}} for the reaction with a {\bf{lower E`a`}}} \tn 
% Row Count 4 (+ 4)
% Row 16
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{fa-long-arrow-down\}\}E`a` = \{\{fa-long-arrow-up\}\}fraction of effective collisions = \{\{fa-long-arrow-up\}\}rate} \tn 
% Row Count 7 (+ 3)
% Row 17
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Rate α \textasciicircum{}`1`\textasciicircum{}/`Ea`}} - as the {\bf{catalyzed activation energy decreases}}, the {\bf{rate increases}}, and vice versa} \tn 
% Row Count 10 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{1.14471 cm} x{3.83229 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Rate Law}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Mathematical relationship}} between the {\bf{reaction rate}} and the {\bf{concentration}} of reactants; needs {\bf{experimental data}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Formula:}} Rate = k{[}A{]}\textasciicircum{}a\textasciicircum{}{[}B{]}\textasciicircum{}b\textasciicircum{}{[}C{]}\textasciicircum{}c\textasciicircum{}} \tn 
% Row Count 4 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{[}A{]}/{[}B{]}/{[}C{]} = concentration of {\bf{reactants}} (only {\bf{reactants}} are relevant); k = rate constant} \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Orders of Reaction}}} \tn 
% Row Count 7 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Order of reaction:}} the exponent used to describe the relationship between the {\bf{{[} i {]} of a reactant}} and the {\bf{rate of reaction}}; tells us {\bf{how quickly the rate will increase}} when {[}conc{]} increases} \tn 
% Row Count 12 (+ 5)
% Row 5
\SetRowColor{white}
Zero order & Rate = k{[}A{]}\textasciicircum{}0\textasciicircum{}; slope is {\bf{flat}}; rate is not affected by {[}A{]} \tn 
% Row Count 15 (+ 3)
% Row 6
\SetRowColor{LightBackground}
First order & Rate = k{[}A{]}\textasciicircum{}1\textasciicircum{}; slope is an {\bf{increasing straight}} line; rate α {[}A{]} \tn 
% Row Count 18 (+ 3)
% Row 7
\SetRowColor{white}
Second order & Rate = k{[}A{]}\textasciicircum{}2\textasciicircum{}; slope is an {\bf{increasing curve}}; rate α {[}A{]}\textasciicircum{}2\textasciicircum{} \tn 
% Row Count 21 (+ 3)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Total order of reaction}} = the {\bf{sum}} of the exponents in the rate law equation} \tn 
% Row Count 23 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{The only accurate data for concentration and rate is the {\bf{initial rate}}, because as soon as the reaction starts, products are formed and the {\bf{reverse reaction starts}}, making any rate measured after {\emph{t}} = 0 affected by the products.}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Reaction Mechanisms}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Chemical reactions usually occur as a {\bf{sequence}} of {\bf{elementary steps}} that, when added, result in the {\bf{overall reaction}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Mechanism is dependent on the slowest elementary step - the {\bf{rate-determining step}}} \tn 
% Row Count 5 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Elementary step}} = a single molecular event in the reaction mechanism} \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{3 criteria for a proposed reaction mechanism:}}} \tn 
% Row Count 9 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{The elementary steps must {\bf{add up to the overall reaction}}} \tn 
% Row Count 11 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{The elementary steps must {\bf{be physically reasonable}} - there should not be more than 2 reactants} \tn 
% Row Count 13 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{The rate-determining step must {\bf{be consistent with the rate law equation}}} \tn 
% Row Count 15 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


% That's all folks
\end{multicols*}

\end{document}