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% Document Info
\author{kaliap714}
\pdfinfo{
  /Title (rice-chem-122-formula-info-sheet.pdf)
  /Creator (Cheatography)
  /Author (kaliap714)
  /Subject (Rice CHEM 122 Formula/Info Sheet 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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\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Rice CHEM 122 Formula/Info Sheet Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{kaliap714} via \textcolor{DarkBackground}{\uline{cheatography.com/36789/cs/11570/}}}
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\noindent
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\begin{tabulary}{5.8cm}{LL}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}kaliap714 \\
  \uline{cheatography.com/kaliap714} \\
  \end{tabulary}
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 26th April, 2017.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\begin{document}
\raggedright
\raggedcolumns

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% www.emerson.emory.edu/services/latex/latex_169.html
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\begin{multicols*}{4}

\begin{tabularx}{3.833cm}{x{1.78516 cm} x{1.64784 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{UNIT 1}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\bf{Formula Name}} & {\bf{Equation}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Boyle's Law & PV = k (N,T) \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
Charles's Law & V/T = k (N,P) \tn 
% Row Count 3 (+ 1)
% Row 3
\SetRowColor{white}
Avogadro's Law & V/n = k (T,P) \tn 
% Row Count 4 (+ 1)
% Row 4
\SetRowColor{LightBackground}
Ideal Gas Law & V = nRT/P or PV = nRT \tn 
% Row Count 6 (+ 2)
% Row 5
\SetRowColor{white}
Dalton's Law & Ptotal = P1 + P2 + P3.... \tn 
% Row Count 8 (+ 2)
% Row 6
\SetRowColor{LightBackground}
STP & 1 atm, 0 Celsius \tn 
% Row Count 9 (+ 1)
% Row 7
\SetRowColor{white}
Gas Density & d = m/V = PM/RT = N/V \tn 
% Row Count 11 (+ 2)
% Row 8
\SetRowColor{LightBackground}
Partial Pressure & P1 = X1 * Ptotal \tn 
% Row Count 12 (+ 1)
% Row 9
\SetRowColor{white}
Root Mean Squared Speed & v = sqrt(3RT/M) \tn 
% Row Count 14 (+ 2)
% Row 10
\SetRowColor{LightBackground}
Collision Frequency & f = vrms / mfp (mean free path) \tn 
% Row Count 16 (+ 2)
% Row 11
\SetRowColor{white}
Average Kinetic Energy & KE = 3/2 nRT \tn 
% Row Count 18 (+ 2)
% Row 12
\SetRowColor{LightBackground}
Effusion - Graham's Law & rate1/rate2 = sqrt(MW2/MW1) \tn 
% Row Count 20 (+ 2)
% Row 13
\SetRowColor{white}
General Rate Law & rate = k{[}A{]}\textasciicircum{}m*{[}B{]}\textasciicircum{}n \tn 
% Row Count 21 (+ 1)
% Row 14
\SetRowColor{LightBackground}
Zeroth Order Integrated Rate Law & {[}A{]}t = {[}A{]}0 - kt \tn 
% Row Count 23 (+ 2)
% Row 15
\SetRowColor{white}
First Order Integrated Rate Law & ln{[}A{]}t = ln{[}A{]}0 -kt \tn 
% Row Count 25 (+ 2)
% Row 16
\SetRowColor{LightBackground}
Second Order Integrated Rate LAw & 1/{[}A{]}t = 1/{[}A{]}0 + kt \tn 
% Row Count 27 (+ 2)
% Row 17
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Zeroth Order Half Life & t = {[}A{]}0/2k \tn 
% Row Count 29 (+ 2)
% Row 18
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First Order Half Life & t = ln2/k \tn 
% Row Count 31 (+ 2)
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\par\addvspace{1.3em}

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% Row 19
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Second Order Half Life & t = 1/k{[}A{]}0 \tn 
% Row Count 2 (+ 2)
% Row 20
\SetRowColor{white}
Arrhenius Equation & Ae\textasciicircum{}-Ea/RT \tn 
% Row Count 3 (+ 1)
% Row 21
\SetRowColor{LightBackground}
Logarithmic Form of Arrhenius Equation & ln(k2/k1) = (-Ea/R) * (1/T2 - 1/T1) \tn 
% Row Count 5 (+ 2)
% Row 22
\SetRowColor{white}
Michaelis-Menton Enzyme Kinetics & rate = k2 {[}E{]}T {[}S{]}/{[}S{]} + km \tn 
% Row Count 7 (+ 2)
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% Row 0
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{\bf{Formula Name/Subject}} & {\bf{Equation/Description}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Equilibrium Constant (concentrations) & Kc = {[}products{]}/{[}reactants{]} \tn 
% Row Count 4 (+ 2)
% Row 2
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Equilibrium Constant (pressures) & Kp = \seqsplit{P(products)/P(reactants)} \tn 
% Row Count 6 (+ 2)
% Row 3
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Equilibrium Equation (with rates) & K = kf/kr \tn 
% Row Count 8 (+ 2)
% Row 4
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Q = K & At equilibirum \tn 
% Row Count 9 (+ 1)
% Row 5
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Q \textless{} K & reaction shifts in forward direction \tn 
% Row Count 11 (+ 2)
% Row 6
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Q \textgreater{} K & reaction shifts in reverse direction \tn 
% Row Count 13 (+ 2)
% Row 7
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Keq is large (10\textasciicircum{}3) & kforward \textgreater{} kreverse \tn 
% Row Count 14 (+ 1)
% Row 8
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Keq is small (10\textasciicircum{}-3) & kforward \textless{} kreverse \tn 
% Row Count 15 (+ 1)
% Row 9
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Keq = 1 & kforward = kreverse \tn 
% Row Count 16 (+ 1)
% Row 10
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Kc and Kp Relation & Kc = Kp * RT\textasciicircum{}Δn \tn 
% Row Count 17 (+ 1)
% Row 11
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L'C: add more reactants & reaction shifts forward \tn 
% Row Count 19 (+ 2)
% Row 12
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L'C: add more products & reaction shifts reverse \tn 
% Row Count 21 (+ 2)
% Row 13
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L'C: increase pressure & reaction shifts towards fewer moles \tn 
% Row Count 23 (+ 2)
% Row 14
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L'C: decrease pressure & reaction shifts towards greter moles \tn 
% Row Count 25 (+ 2)
% Row 15
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L'C: increase volume & reaction shifts towards greater moles \tn 
% Row Count 27 (+ 2)
% Row 16
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L'C: decrease volume & reaction shifts towards fewer moles \tn 
% Row Count 29 (+ 2)
% Row 17
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Endothermic (T) Phase Transitions & Melting, Sublimation, Evaporation \tn 
% Row Count 31 (+ 2)
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% Row 18
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Exothermic (P) Phase Transitions & Freezing, Deposition, Condensation \tn 
% Row Count 2 (+ 2)
% Row 19
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Entropy & S = kB ln(W) \tn 
% Row Count 3 (+ 1)
% Row 20
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Change in Entropy for Change in Volume & ΔS = nR ln(V2/V1) \tn 
% Row Count 5 (+ 2)
% Row 21
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Change in Entropy ofSurroundings & ΔSsurr = -ΔH/T \tn 
% Row Count 7 (+ 2)
% Row 22
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Gibbs Free Energy & ΔG = ΔH - TΔS \tn 
% Row Count 8 (+ 1)
% Row 23
\SetRowColor{white}
Nonstandard Gibbs Free Energy (1) & ΔG = ΔG0 + RTlnQ \tn 
% Row Count 10 (+ 2)
% Row 24
\SetRowColor{LightBackground}
Standard Gibbs Free Energy & ΔG0 = -RTlnK \tn 
% Row Count 12 (+ 2)
% Row 25
\SetRowColor{white}
Nonstandard Gibbs Free Energy (2) & ΔG = RT ln(Q/K) \tn 
% Row Count 14 (+ 2)
% Row 26
\SetRowColor{LightBackground}
Clausisus-Claperyon Equation & ln(P2/P1) = -ΔH/R (1/T2-1/T1) \tn 
% Row Count 16 (+ 2)
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% Row 0
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{\bf{Formula Name/Info}} & {\bf{Equation/Description}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Molarity (M) & mol solute/L solution (mol/L) \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
Molality (m) & mol solute/kg solution (mol/kg) \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
Mole Fraction (X) & mol solute/mol solution (mol/mol) \tn 
% Row Count 8 (+ 2)
% Row 4
\SetRowColor{LightBackground}
Vapor Pressure (two volatile chemicals) & Pvap = P{\emph{aXa + P}}bXb \tn 
% Row Count 11 (+ 3)
% Row 5
\SetRowColor{white}
Boiling Point Elevation & Tb = kb {\emph{ m }} i \tn 
% Row Count 13 (+ 2)
% Row 6
\SetRowColor{LightBackground}
Freezing Point Depression & Tf = -kf {\emph{ m }} i \tn 
% Row Count 15 (+ 2)
% Row 7
\SetRowColor{white}
Osmotic Pressure & pi  =iMRT \tn 
% Row Count 16 (+ 1)
% Row 8
\SetRowColor{LightBackground}
Solubility & S = mol dissolved / L solution \tn 
% Row Count 18 (+ 2)
% Row 9
\SetRowColor{white}
CIE: add in species already present & decrease solubility \tn 
% Row Count 20 (+ 2)
% Row 10
\SetRowColor{LightBackground}
\seqsplit{Henderson-Hasselbach} Equation & pH = pKa + log(conj. base/acid) \tn 
% Row Count 22 (+ 2)
% Row 11
\SetRowColor{white}
K value for Neutralization & Kn = Ka*Kb/Kw \tn 
% Row Count 24 (+ 2)
% Row 12
\SetRowColor{LightBackground}
Equivalence Point & mol base added = mol acid originally present \tn 
% Row Count 27 (+ 3)
% Row 13
\SetRowColor{white}
Midpoint & pH = pKa \tn 
% Row Count 28 (+ 1)
% Row 14
\SetRowColor{LightBackground}
Solvent-Solvent Interactions & endothermic, overcome IMFs \tn 
% Row Count 30 (+ 2)
\end{tabularx}
\par\addvspace{1.3em}

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\begin{tabularx}{3.833cm}{x{1.68217 cm} x{1.75083 cm} }
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% Row 15
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Solute-Solute Interactions & endothermic, overcome IMFs \tn 
% Row Count 2 (+ 2)
% Row 16
\SetRowColor{white}
Solvent-Solute Interactions & exothermic, release energy through attractive forces \tn 
% Row Count 5 (+ 3)
% Row 17
\SetRowColor{LightBackground}
To relate Ka to Kb & Kw = Ka * Kb \tn 
% Row Count 6 (+ 1)
% Row 18
\SetRowColor{white}
Strong Acids & H2SO4, HNO3, HCl, HI, HClO4, HClO3, HBr \tn 
% Row Count 8 (+ 2)
% Row 19
\SetRowColor{LightBackground}
Strong Bases & LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2 \tn 
% Row Count 11 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{3.833cm}{x{1.54485 cm} x{1.88815 cm} }
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\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{UNIT 4}}  \tn
% Row 0
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{\bf{Formula Name/Subject}} & {\bf{Equation/Description}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
Current (I)) & charge/time (Amperes) \tn 
% Row Count 3 (+ 1)
% Row 2
\SetRowColor{LightBackground}
Voltage (V) & energy/charge (Volts) \tn 
% Row Count 4 (+ 1)
% Row 3
\SetRowColor{white}
Power (W) & energy/seconds (Watts) \tn 
% Row Count 5 (+ 1)
% Row 4
\SetRowColor{LightBackground}
Oxidation Reaction & Lose electrons \tn 
% Row Count 6 (+ 1)
% Row 5
\SetRowColor{white}
Reduction Reaction & Gain electrons \tn 
% Row Count 7 (+ 1)
% Row 6
\SetRowColor{LightBackground}
Cathode & Site of reduction, e- flow to cathode \tn 
% Row Count 9 (+ 2)
% Row 7
\SetRowColor{white}
Anode & Site of oxidation, e- flow from anode \tn 
% Row Count 11 (+ 2)
% Row 8
\SetRowColor{LightBackground}
Cell Potential (E) & Ecell = Ecathode + Eanode = Eredcat - Eredan \tn 
% Row Count 13 (+ 2)
% Row 9
\SetRowColor{white}
Gibbs Free Energy (standard) & ΔG0 = -nFE0 \tn 
% Row Count 15 (+ 2)
% Row 10
\SetRowColor{LightBackground}
Faraday's Constant & 96,500 C/mol e- \tn 
% Row Count 16 (+ 1)
% Row 11
\SetRowColor{white}
Nernst Equation & E = E0 - RT/nF lnQ \tn 
% Row Count 17 (+ 1)
% Row 12
\SetRowColor{LightBackground}
Standard Hydrogen Electrode (SHE) & 2H+ + 2e- -\textgreater{} H2(g) \tn 
% Row Count 19 (+ 2)
% Row 13
\SetRowColor{white}
Standard Cell Potential & E0 = RT/nF lnK \tn 
% Row Count 21 (+ 2)
% Row 14
\SetRowColor{LightBackground}
Total Charge (Z) & Z = I * t (in seconds), in coloumbs \tn 
% Row Count 23 (+ 2)
% Row 15
\SetRowColor{white}
Moles of Electrons Produced & n(e-) = Z/F \tn 
% Row Count 25 (+ 2)
% Row 16
\SetRowColor{LightBackground}
Moles of Metal Produced & n(metal) = n(e-)* mol(metal)/mols e- needed \tn 
% Row Count 27 (+ 2)
% Row 17
\SetRowColor{white}
Mass of Metal Produced & m(metal) = n(metal)/MWmetal \tn 
% Row Count 29 (+ 2)
% Row 18
\SetRowColor{LightBackground}
Nernst Equation with pH & E = E0red + 2.3RT/F logQ \tn 
% Row Count 31 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}