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\author{TheGoldenClover}
\pdfinfo{
  /Title (tahsili-chemistry-reaction-rates-and-equilibrium.pdf)
  /Creator (Cheatography)
  /Author (TheGoldenClover)
  /Subject (Tahsili Chemistry (Reaction Rates and Equilibrium) Cheat Sheet)
}

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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Tahsili Chemistry (Reaction Rates and Equilibrium) Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{TheGoldenClover} via \textcolor{DarkBackground}{\uline{cheatography.com/201551/cs/42788/}}}
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  \vspace{-2pt}TheGoldenClover \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 20th March, 2024.\\
   Updated 20th March, 2024.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
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\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{x{3.28 cm} x{4.72 cm} }
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Rate Of Reaction}}  \tn
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Rate & - ΔReactants / Δt = Δproducts / Δt \tn 
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\mymulticolumn{2}{x{8.4cm}}{Reactants are {\emph{negative}}} \tn 
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Collision Theory & states that particles must collide for a reaction to occur, and must have the right orientation and enough energy \tn 
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Activated Complex & a complex that exists very briefly in the time between the breaking down of reactants and forming of products \tn 
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% Row 4
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Activation Energy & the minimum amount of energy needed to form the activated complex \tn 
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Exothermic Reaction & a reaction that releases energy; the products end up having less energy that the reactants \tn 
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Endothermic reaction & a reaction that must absorb enough energy to overcome the energy barrier; the products have more energy at the end \tn 
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Factors that affect the rate & catalysts - the nature of the substances - Concentration - Surface Area - Temperature \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Factors Affecting Equilibrium}}  \tn
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Characteristics of equilibrium & 1- fixed ratio, 2- closed system, 3-fixed temp, 4- dynamic equilibrium \tn 
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% Row 1
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Le Chatelier's Principle & a change in one variable that describes a system produces a shift in the position of the equilibrium, countering the change \tn 
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Effects of Changing Concentration: & higher reactant concentration = reaction shifts to the right, and vice versa \tn 
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Effects of Changing Temperature & adding heat to and exothermic reaction = more reactants; adding heat to an endothermic reaction = more products \tn 
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Effects of Changing Pressure and Volume & Higher pressure + lower volume = lower number of moles; lower pressure + higher volume = more moles \tn 
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\mymulticolumn{2}{x{8.4cm}}{{\emph{if the number of moles are equal on both sides, pressure and volume will have no effect}}} \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Rate Law}}  \tn
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Rate Law & R = k {[}A{]}\textasciicircum{}x\textasciicircum{} {[}B{]}\textasciicircum{}y\textasciicircum{} \tn 
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Order of the reaction & x+y \tn 
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Rate Constant (k) & is only affected by temp \tn 
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Rate Constant Units & s\textasciicircum{}-1\textasciicircum{} , L/mol.s , L\textasciicircum{}2\textasciicircum{}/mol\textasciicircum{}2\textasciicircum{}.s \tn 
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\mymulticolumn{2}{x{8.4cm}}{A and B are the molar concentrations of reactants; the rate is directly proportional to the concentrations} \tn 
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\mymulticolumn{2}{x{8.4cm}}{the coefficients are the exponents} \tn 
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Complete Reaction & when reactants change to products (→) \tn 
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Reversible reaction & can go both ways (⇆) \tn 
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Equilibrium & when the rate of the forward reaction equals the rate of the backwards one \tn 
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Chemical Equilibrium Law & states that at a certain temperature, the ratio of the reactants and products can remain constant \tn 
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Chemical Equilibrium Law Formula & K eq = {[}C{]}\textasciicircum{}c\textasciicircum{}{[}D{]}\textasciicircum{}d\textasciicircum{} / {[}A{]}\textasciicircum{}a\textasciicircum{}{[}B{]}\textasciicircum{}b\textasciicircum{} \tn 
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Homogeneous Equilibrium & when the reactants and products are in the same state of matter \tn 
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Heterogeneous Equilibrium & when the reactants and products are in multiple states (the pure solid and liquids are removed from the equation) \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Temperature and The Equilibrium Constant}}  \tn
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K eq is directly proportional to temp id the equation is: & endothermic \tn 
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K eq is inversely proportional to temp id the equation is: & exothermic \tn 
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catalyst & increases the speed at which a reaction reaches equilibrium, but does not change the equilibrium \tn 
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\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Temperature and The Equilibrium Constant}}  \tn
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K eq is directly proportional to temp id the equation is: & \seqsplit{endothermic} \tn 
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K eq is inversely proportional to temp id the equation is: & \seqsplit{exothermic} \tn 
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% That's all folks
\end{multicols*}

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