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% Document Info
\author{Tana}
\pdfinfo{
  /Title (0620-chemistry-carbonates.pdf)
  /Creator (Cheatography)
  /Author (Tana)
  /Subject (0620 Chemistry Carbonates Cheat Sheet)
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\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{0620 Chemistry Carbonates Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{Tana} via \textcolor{DarkBackground}{\uline{cheatography.com/144948/cs/31857/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}Tana \\
  \uline{cheatography.com/tana} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 26th April, 2022.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\begin{document}
\raggedright
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% from this page to resize cheat sheet text:
% www.emerson.emory.edu/services/latex/latex_169.html
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\begin{tabularx}{17.67cm}{p{1.727 cm} p{1.727 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{17.67cm}}{\bf\textcolor{white}{Manufacture of lime}}  \tn
% Row 0
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\mymulticolumn{2}{x{17.67cm}}{{\bf{{\emph{Lime}}}}} \tn 
% Row Count 1 (+ 1)
% Row 1
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\mymulticolumn{2}{x{17.67cm}}{• Limestone consists of calcium carbonate, CaCO₃} \tn 
% Row Count 3 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{• Lime (calcium oxide) is manufactured from calcium carbonate by {\emph{thermal decomposition}}} \tn 
% Row Count 5 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{17.67cm}}{CaO + H₂O → CaO + CO₂} \tn 
% Row Count 6 (+ 1)
% Row 4
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\mymulticolumn{2}{x{17.67cm}}{{\bf{{\emph{Slaked lime (calcium hydroxide)}}}}} \tn 
% Row Count 7 (+ 1)
% Row 5
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\mymulticolumn{2}{x{17.67cm}}{• It is made by adding a small amount of water slowly to calcium oxide} \tn 
% Row Count 9 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{CaO + H₂O → Ca(OH)₂} \tn 
% Row Count 10 (+ 1)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{17.67cm}}{→Limewater is a solution of calcium hydroxide in water (hence it is alkaline)} \tn 
% Row Count 12 (+ 2)
% Row 8
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\mymulticolumn{2}{x{17.67cm}}{{\bf{{\emph{Addition of CO₂}}}}} \tn 
% Row Count 13 (+ 1)
% Row 9
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\mymulticolumn{2}{x{17.67cm}}{• Addition of carbon dioxide to calcium hydroxide produces, calcium carbonate} \tn 
% Row Count 15 (+ 2)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{→ This reaction is the basis of the standard chemical test for CO₂} \tn 
% Row Count 17 (+ 2)
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\par\addvspace{1.3em}

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\mymulticolumn{1}{x{17.67cm}}{\bf\textcolor{white}{Limestone cycle}}  \tn
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\mymulticolumn{1}{p{17.67cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/tana_1650954922_limestone cycle.png}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\mymulticolumn{1}{x{17.67cm}}{The combination of the three reaction above constitute the limestone cycle}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\par\addvspace{1.3em}

\begin{tabularx}{17.67cm}{p{1.727 cm} p{1.727 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{17.67cm}}{\bf\textcolor{white}{Uses of quick lime}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{• Making steel from iron} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{17.67cm}}{• To neutralize acidity in soil} \tn 
% Row Count 2 (+ 1)
% Row 2
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\mymulticolumn{2}{x{17.67cm}}{• Drying agent in industry} \tn 
% Row Count 3 (+ 1)
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\begin{tabularx}{17.67cm}{p{1.727 cm} p{1.727 cm} }
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\mymulticolumn{2}{x{17.67cm}}{\bf\textcolor{white}{Uses of slaked lime and lime}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{• Neutralize acidity in soil and lakes affected in soil} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{17.67cm}}{• Neutralizing acidic industrial waste products (flue gas desulphurization)} \tn 
% Row Count 4 (+ 2)
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\par\addvspace{1.3em}

\begin{tabularx}{17.67cm}{p{1.727 cm} p{1.727 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{17.67cm}}{\bf\textcolor{white}{Uses of limestone (CaCO₃)}}  \tn
% Row 0
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\mymulticolumn{2}{x{17.67cm}}{{\bf{Making cement}}} \tn 
% Row Count 1 (+ 1)
% Row 1
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\mymulticolumn{2}{x{17.67cm}}{• Manufactured by heating a mixture of powdered limestone and clay in rotary kiln. Once heated, calcium sulfate and water are added which produce cement} \tn 
% Row Count 5 (+ 4)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{→ Adding gypsum (calcium sulfate) and grinding up the final solid to give a powder} \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{17.67cm}}{{\bf{Making iron}}} \tn 
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% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{17.67cm}}{• Limestone is added to blast furnace where it decomposes to form lime (CaO) and carbon dioxide. The lime reacts with silica impurities to form calcium silicate (slag), which floats to the top of the molten iron and is removed and is then used for road building} \tn 
% Row Count 14 (+ 6)
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