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% Most of the following are not required for the majority
% of cheat sheets but are needed for some symbol support.
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% Document Info
\author{resaraj}
\pdfinfo{
  /Title (termochemistry.pdf)
  /Creator (Cheatography)
  /Author (resaraj)
  /Subject (Termochemistry Cheat Sheet)
}

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\fancyhead[L]{
\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{C}
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    \vspace{-7pt}
    {\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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\columnbreak
\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Termochemistry Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{resaraj} via \textcolor{DarkBackground}{\uline{cheatography.com/209482/cs/45062/}}}
\end{tabulary}
\end{multicols}}

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\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{LL}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}resaraj \\
  \uline{cheatography.com/resaraj} \\
  \end{tabulary}
\vfill
\columnbreak
\begin{tabulary}{5.8cm}{L}
  \SetRowColor{FootBackground}
  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 20th November, 2024.\\
   Page {\thepage} of \pageref{LastPage}.
\end{tabulary}
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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
\end{tabulary}
\end{multicols}}




\begin{document}
\raggedright
\raggedcolumns

% Set font size to small. Switch to any value
% from this page to resize cheat sheet text:
% www.emerson.emory.edu/services/latex/latex_169.html
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\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Systems}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{A system can be open (freely exchanges energy and matter with the surroundings), closed (exchanges energy but not matter) or insulated (does not interact with the surroundings)} \tn 
% Row Count 4 (+ 4)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Sign conventions}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{8.4cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/resaraj_1732103668_Captura de pantalla 2024-11-20 125231.png}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{If the system gains heat, it is an endothermic process. If the system releases heat, it is an exothermic process.}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{3.52 cm} x{4.48 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Heat}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\emph{Q=m•Hs•ΔT}} & not a state function \tn 
% Row Count 1 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{4.4 cm} x{3.6 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Work}}  \tn
% Row 0
\SetRowColor{LightBackground}
pressure-volume work & {\emph{W=Pext•V}} (if P=constant) \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
if carried out in a reversible way & {\emph{W=-nRT•ln(V2/V1)}} \tn 
% Row Count 4 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{2.48 cm} x{5.52 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Ideal gas law}}  \tn
% Row 0
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{\emph{P•V=nRT}} & R=0,082 atm•L/(K•mol) \tn 
% Row Count 1 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{p{4 cm} p{4 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Calorimeter bomb}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{{\emph{Q+W=0=ΔE}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
W=0 & Q=0 \tn 
% Row Count 2 (+ 1)
% Row 2
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\mymulticolumn{2}{x{8.4cm}}{Qreleased+Qabsorbed=0} \tn 
% Row Count 3 (+ 1)
% Row 3
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\mymulticolumn{2}{x{8.4cm}}{\seqsplit{Qreaction+Qwater+Qcalorimeter=0}} \tn 
% Row Count 4 (+ 1)
% Row 4
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\mymulticolumn{2}{x{8.4cm}}{\seqsplit{Qreaction+Mwater•(Tf-Ti)+Kcalorimeter•(Tf-Ti)=0}} \tn 
% Row Count 6 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{8.4cm}}{Qreaction=Qv=ΔE} \tn 
% Row Count 7 (+ 1)
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\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{p{0.8 cm} p{0.8 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Laws of thermochemistry}}  \tn
% Row 0
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\mymulticolumn{2}{x{8.4cm}}{{\bf{Lavoisier and Laplace laws}}} \tn 
% Row Count 1 (+ 1)
% Row 1
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\mymulticolumn{2}{x{8.4cm}}{The energy change accompanying any transformation is equal and opposite to energy change accompanying the reverse process.} \tn 
% Row Count 4 (+ 3)
% Row 2
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\mymulticolumn{2}{x{8.4cm}}{{\bf{Hess Law}}} \tn 
% Row Count 5 (+ 1)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{8.4cm}}{The energy change accompanying any transformation is the same whether the process occurs in one step or many. The combination of chemical equations allows to determine unknown heats of reaction.} \tn 
% Row Count 9 (+ 4)
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\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{p{0.8 cm} p{0.8 cm} }
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Standard States. Standard enthalpy of reaction}}  \tn
% Row 0
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\mymulticolumn{2}{x{8.4cm}}{enthalpy change of a reaction in which all reactants and products are in their standard states} \tn 
% Row Count 2 (+ 2)
% Row 1
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\mymulticolumn{2}{x{8.4cm}}{the standard enthalpy of formation of a pure element in its standard state is 0} \tn 
% Row Count 4 (+ 2)
% Row 2
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\mymulticolumn{2}{x{8.4cm}}{\seqsplit{ΔHº=Σvp•ΔHºf(products)-Σvp•ΔHºf(reactants)}} \tn 
% Row Count 6 (+ 2)
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\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{2 cm} x{6 cm} }
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Units}}  \tn
% Row 0
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\mymulticolumn{2}{x{8.4cm}}{1cal=4,184J} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Specific heat & quantity of heat required to change the temperature of one gram of the substance by one degree celsius \tn 
% Row Count 5 (+ 4)
% Row 2
\SetRowColor{LightBackground}
Molar heat & quantity of heat required to change the temperature of one mol of the substance by one degree celsius \tn 
% Row Count 9 (+ 4)
% Row 3
\SetRowColor{white}
Heat capacity & quantity of heat required to change the temperature of a system by one degree celsius \tn 
% Row Count 12 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{6.24 cm} x{1.76 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{First law of thermodynamics}}  \tn
% Row 0
\SetRowColor{LightBackground}
Internal energy is the total energy in a system & {\emph{E=ΣEi}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Principle of conservation of energy & {\emph{ΔE=Q+W}} \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
For isolated system & {\emph{Q+W=0=ΔE}} \tn 
% Row Count 6 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{Heat and work are means by which a system exchanges energy with the surroundings}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{4.32 cm} x{3.68 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Enthalpy (H)}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{It is the change in the internal energy when there is only pressure-volume work, and the pressure is constant} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
{\emph{ΔE=Q+W=Qp-P•ΔV}} & {\emph{Qp=ΔE+P•ΔV}} \tn 
% Row Count 4 (+ 1)
% Row 2
\SetRowColor{LightBackground}
H=E+P•V & {\emph{ΔH=ΔE+VΔP+PΔV +ΔPΔV}} \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
if P=constant & {\emph{ΔH=Qp=m•Hs•ΔT=n•Hs•ΔT}} \tn 
% Row Count 8 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{{\bf{Relation of Qv and Qp (gases)}}} \tn 
% Row Count 9 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{8.4cm}}{{\emph{ΔH=ΔE+PΔV}}} \tn 
% Row Count 10 (+ 1)
% Row 6
\SetRowColor{LightBackground}
if P and T are constant & {\emph{ΔH=ΔE+ΔnRT}} \tn 
% Row Count 12 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{8.4cm}}{{\bf{Relation of Qv and Qp (solids and liquids)}}} \tn 
% Row Count 13 (+ 1)
% Row 8
\SetRowColor{LightBackground}
if P=constant-{}-\textgreater{}change in volume really small & {\emph{Qv≈Qp-{}-\textgreater{}ΔE≈ΔH}} \tn 
% Row Count 16 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Enthalpy and bond energy}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{ΔHr=ΣHbroken bonds-ΣHformed bonds} \tn 
% Row Count 1 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}