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% Document Info
\author{TheGoldenClover}
\pdfinfo{
  /Title (tahsili-chemistry-chemical-calculations.pdf)
  /Creator (Cheatography)
  /Author (TheGoldenClover)
  /Subject (Tahsili Chemistry (Chemical Calculations) Cheat Sheet)
}

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\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{C}
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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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\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Tahsili Chemistry (Chemical Calculations) Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{TheGoldenClover} via \textcolor{DarkBackground}{\uline{cheatography.com/201551/cs/42700/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}TheGoldenClover \\
  \uline{cheatography.com/thegoldenclover} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 12th March, 2024.\\
   Updated 12th March, 2024.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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% Set font size to small. Switch to any value
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\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{x{2.64 cm} x{5.36 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Moles}}  \tn
% Row 0
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Avogadro's number & 6.02 x 10\textasciicircum{}23\textasciicircum{} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Molar Mass & the mass of one mol of a substance \tn 
% Row Count 4 (+ 2)
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\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{3.68 cm} x{4.32 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Gas Laws}}  \tn
% Row 0
\SetRowColor{LightBackground}
Boyle's Law (Constant Temp) & P1V1 = P2V2 \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Graph Shape & a decreasing curve \tn 
% Row Count 3 (+ 1)
% Row 2
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Charle's Law (Constant Pressure) & V1/T1 = V2/T2 \tn 
% Row Count 5 (+ 2)
% Row 3
\SetRowColor{white}
Graph Shape & an increasing line \tn 
% Row Count 6 (+ 1)
% Row 4
\SetRowColor{LightBackground}
Gay-Lussac's Law (Constant Volume) & P1/T1 = P2/T2 \tn 
% Row Count 8 (+ 2)
% Row 5
\SetRowColor{white}
Graph Shape & an increasing line \tn 
% Row Count 9 (+ 1)
% Row 6
\SetRowColor{LightBackground}
General Law & P1V1/T1 = P2V2/T2 \tn 
% Row Count 10 (+ 1)
% Row 7
\SetRowColor{white}
Ideal Gas Law & PV = nRT (R = 0.082) \tn 
% Row Count 11 (+ 1)
% Row 8
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Standard Conditions (STP) & temp = 273 K / 0 C and P = 1 atm \tn 
% Row Count 13 (+ 2)
% Row 9
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Avogadro's Principle & equal volumes of gases have equal number of particles at the same temp and pressure \tn 
% Row Count 17 (+ 4)
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\begin{tabularx}{8.4cm}{x{3.92 cm} x{4.08 cm} }
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Chemical Potential Energy and Heat}}  \tn
% Row 0
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Chemical Potential Energy & the stored energy in the structure of matter \tn 
% Row Count 3 (+ 3)
% Row 1
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Heat & the energy transferred between objects (Joules) \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
Calorie & the amount of energy required to raise 1 gram of water by 1 degree C \tn 
% Row Count 10 (+ 4)
% Row 3
\SetRowColor{white}
Heat Content (H) & the amount of stored heat energy per mol under constant pressure \tn 
% Row Count 14 (+ 4)
% Row 4
\SetRowColor{LightBackground}
Change in Heat Content / Enthalpy (ΔH) & the energy absorbed or released in a reaction \tn 
% Row Count 17 (+ 3)
% Row 5
\SetRowColor{white}
Enthalpy Formula & ΔH = H (products) - H (reactants) \tn 
% Row Count 19 (+ 2)
% Row 6
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H (products) \textless{} H (reactants) & the reaction is exothermic, and will have a negative value \tn 
% Row Count 22 (+ 3)
% Row 7
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H (products) \textgreater{} H (reactants) & the reaction is endothermic, and will have a positive value \tn 
% Row Count 25 (+ 3)
% Row 8
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Hess's law & states that regardless of the multiple stages, the total enthalpy change is the sum of all the changes \tn 
% Row Count 31 (+ 6)
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Chemical Potential Energy and Heat (cont)}}  \tn
% Row 9
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Standard heat of formation & The change in heat content when 1 mol of compound is formed from its elements in standard conditions \tn 
% Row Count 5 (+ 5)
% Row 10
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\mymulticolumn{2}{x{8.4cm}}{{\emph{endothermic = positive = cold reactions}}} \tn 
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% Row 11
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% Row 12
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Empirical and Molecular Formulas}}  \tn
% Row 0
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Percent composition of A in AB & ( Mass of A / Mass of AB ) x 100\% \tn 
% Row Count 2 (+ 2)
% Row 1
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Empirical Formula & The simplest whole number ratio of atoms (Ex: CH) \tn 
% Row Count 5 (+ 3)
% Row 2
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Molecular Formula & The actual number of atoms in a molecule (Ex: C6H6) \tn 
% Row Count 8 (+ 3)
% Row 3
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N whole Number & N = molecular formula mass / empirical formula mass \tn 
% Row Count 11 (+ 3)
% Row 4
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Hydrated Salts & salts with water molecules in it's crystals \tn 
% Row Count 13 (+ 2)
% Row 5
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\mymulticolumn{2}{x{8.4cm}}{{\emph{when hydrated salts are heated, they lose their water}}} \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Calculations In Gases}}  \tn
% Row 0
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Limiting Reactant & the substance that is used up completely \tn 
% Row Count 2 (+ 2)
% Row 1
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Excess Reactant & the substance that is not used up and remains after the reaction \tn 
% Row Count 5 (+ 3)
% Row 2
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Theoretical yield & the largest amount of product that can be produced \tn 
% Row Count 7 (+ 2)
% Row 3
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Actual Yield & the amount produced by the experiment \tn 
% Row Count 9 (+ 2)
% Row 4
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Percent Yield & = (actual yield / theoretical yield) x 100 \tn 
% Row Count 11 (+ 2)
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% Row 0
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\mymulticolumn{1}{x{8.4cm}}{a gas is comprised of molecules whose {\bf{average distance}} between each other is {\bf{greater than the size of its particles}}} \tn 
% Row Count 3 (+ 3)
% Row 1
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% Row Count 5 (+ 2)
% Row 2
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\mymulticolumn{1}{x{8.4cm}}{The particles are in {\bf{constant random motion}}} \tn 
% Row Count 6 (+ 1)
% Row 3
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\mymulticolumn{1}{x{8.4cm}}{The KE of a particle depends on its {\bf{mass and velocity}}} \tn 
% Row Count 8 (+ 2)
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Gas Behavior}}  \tn
% Row 0
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Diffusion & the movement of particles from areas of high concentration to areas of low concentration \tn 
% Row Count 4 (+ 4)
% Row 1
\SetRowColor{white}
Graham's Law of Diffusion & Rate1 / Rate2 = √(molar mass 2 / molar mass 1) \tn 
% Row Count 6 (+ 2)
% Row 2
\SetRowColor{LightBackground}
Flowing & the movement of gases through small holes \tn 
% Row Count 8 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\par\addvspace{1.3em}

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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Pressure}}  \tn
% Row 0
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Pressure & the force applied perpendicularly to the surface of an object per unit area \tn 
% Row Count 4 (+ 4)
% Row 1
\SetRowColor{white}
SI unit & Pascal (N/m\textasciicircum{}2\textasciicircum{}) \tn 
% Row Count 5 (+ 1)
% Row 2
\SetRowColor{LightBackground}
Barometer & measures atmospheric pressure \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
Manometer & measures the pressure of a trapped gas \tn 
% Row Count 9 (+ 2)
% Row 4
\SetRowColor{LightBackground}
Dalton's Law of partial pressure & the total pressure of a mixture of gases is equal to the sum of the individual pressures \tn 
% Row Count 13 (+ 4)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}