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% Document Info
\author{Maryam.Razvi}
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  /Title (stoichiometry-ib-chem-chapter-1.pdf)
  /Creator (Cheatography)
  /Author (Maryam.Razvi)
  /Subject (Stoichiometry (IB Chem Chapter 1) Cheat Sheet)
}

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        \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{Stoichiometry (IB Chem Chapter 1) Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{Maryam.Razvi} via \textcolor{DarkBackground}{\uline{cheatography.com/181035/cs/37643/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}Maryam.Razvi \\
  \uline{cheatography.com/maryam-razvi} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 12th March, 2023.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Formulas}}  \tn
% Row 0
\SetRowColor{LightBackground}
No. of molecules = n {[}no. of moles{]} x A {[}Avogadro's Constant{]} & No. of moles (n) = Mass (m)/ Molar Mass (Mr) \tn 
% Row Count 4 (+ 4)
% Row 1
\SetRowColor{white}
No. of Atoms = No. of Molecules {[}n x A{]} x Atomicity & No. of moles (n) = Volume (dm3) / Molar volume (STP or RTP) \tn 
% Row Count 7 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\% yield = {[}Experimental yield/ Theoretical Yield{]} x 100 & C {[}molarity{]} = no. of moles {[}n{]}/ Volume of concentration {[}v{]} \tn 
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% Row 3
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Ideal Gas Law - PV = nRT & \seqsplit{Volume/concentration} constant - C1V1 = C2V2 \tn 
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\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Finding Percentage Yield of a Reaction}}  \tn
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\mymulticolumn{1}{x{5.377cm}}{Note: \% yield always applies on PRODUCTS} \tn 
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\mymulticolumn{1}{x{5.377cm}}{1: In any situation, first determine which of the products is the limiting reagent} \tn 
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\mymulticolumn{1}{x{5.377cm}}{2: Using the compound which is limiting, form a ration such that {[}limiting reactant : product{]}} \tn 
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\mymulticolumn{1}{x{5.377cm}}{3: Under the ratio, write the coefficient ratio of reactant : product} \tn 
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\mymulticolumn{1}{x{5.377cm}}{4: Add the molar mass OF 1 MOLE} \tn 
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\mymulticolumn{1}{x{5.377cm}}{5: Multiply the Molar mass with the number of moles = mass value} \tn 
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\mymulticolumn{1}{x{5.377cm}}{6: Cross multiply to find the THEORETICAL YIELD} \tn 
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\mymulticolumn{1}{x{5.377cm}}{7: Use the mass of the product given in the question - (EXPERIMENTAL YIELD)} \tn 
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\mymulticolumn{1}{x{5.377cm}}{8: Substitute in the formula: {\bf{{[}Experimental Yield/ Theoretical Yield{]} x 100}} to find \% yield} \tn 
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\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{How to Find the Limiting Reagent}}  \tn
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\mymulticolumn{1}{x{5.377cm}}{Step 1: Write down the whole equation} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 2: Balance the entire equation} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 3: Using the balanced equation, determine the coefficient ratio of the reactants} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 4: Write down the ratios of the values given in the question} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 5: Convert the amounts to moles} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 6: divide the values (mole ratio / coefficient ratio)} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Ans: The smallest value is the limiting reagent} \tn 
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Ideal Gas Law}}  \tn
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\mymulticolumn{1}{x{5.377cm}}{{\bf{PV = nRT}}; where} \tn 
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\mymulticolumn{1}{x{5.377cm}}{P - Pressure (Pa)} \tn 
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\mymulticolumn{1}{x{5.377cm}}{V = Volume (m\textasciicircum{}3\textasciicircum{})} \tn 
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\mymulticolumn{1}{x{5.377cm}}{T - Temperature (K) *Take celsius value and + 273} \tn 
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\mymulticolumn{1}{x{5.377cm}}{R - Constant (8.31 JK/mol)} \tn 
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\mymulticolumn{1}{x{5.377cm}}{n - no. of moles (mol)} \tn 
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Molar Volume Values}}  \tn
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STP - Standard Temperature and Pressure & RTP - Room Temperature and Pressure \tn 
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Temp.: 0 degrees Celsius & Temp.: 20 degrees Celsius \tn 
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Pressure: 1 atm & Pressure = approx. 1atm \tn 
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Volume: 22.7 dm3 & Volume: 24 dm3 \tn 
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Ideal Gas vs. Real Gas}}  \tn
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{\bf{Ideal Gas}} & {\bf{Real Gas}} \tn 
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Obeys all gas laws & All properties change \tn 
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{\emph{No forces of attraction}} & Forces of attraction \tn 
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Collide in straight lines & Collision in random motion \tn 
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\mymulticolumn{2}{x{5.377cm}}{No mass or volume} \tn 
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High Temperature & Low Temperature \tn 
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Low Pressure & High Pressure \tn 
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High Volume & Low Volume \tn 
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Steps to Find a Standard Solution}}  \tn
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\mymulticolumn{1}{x{5.377cm}}{{\bf{Standard Solution}}: a solution of accurately known concentration} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 1: Weigh a known amount of solute} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 2: Dissolve the Solute in a minimal amount of water} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 3: Transfer the solution to a volumetric flask without washing} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 4: Make the solution fill the flask till the meniscus reaches accurate value} \tn 
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\mymulticolumn{1}{x{5.377cm}}{Step 5: Place stopper and invert into mix solution} \tn 
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\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\par\addvspace{1.3em}


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

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