MassTransfer/appendix.tex at master · NanoScaleDesign/MassTransfer · GitHub

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\newpage
\section{Partial pressure and humidity}

\subsection*{Challenge}
If the saturation pressure of water in air at a given temperature is \SI{0.02}{\bar} and the relative humidity of the air is 30\%, calculate the partial pressure of the water vapour in the air.

\subsection*{Solution}
X = Your solution\\
Form: Decimal, to 3 decimal places\\
Place the indicated letter in front of the number\\
Example: aX where $X=42.544$ is entered as \href{http://www.wolframalpha.com/input/?i=md5+hash+of+\%22a42.544\%22}{a42.544}

hash of dX = f8dcaa


\newpage
\section{Pressure and molar density}

\subsection*{Challenge}
Given that the saturation pressure of water in air at a given temperature is \SI{0.05}{\bar} with a saturated molar density of \SI{5}{\kmol\per\cubic\meter}, if the partial pressure of water in the air is \SI{0.01}{\bar}, calculate the molar density of the water in the air.

\subsection*{Solution}
X = Your solution\\
Form: Decimal, to 1 decimal place\\
Place the indicated letter in front of the number\\
Example: aX where $X=42.5$ is entered as \href{http://www.wolframalpha.com/input/?i=md5+hash+of+\%22a42.544\%22}{a42.5}

hash of eX = 1c8d37


\newpage
\section{Specific volume}

\subsection*{Challenge}
Referring to the specific volume of saturated water at 290 K in table A-6 ($v_g$), what is the saturated molar concentration? You cannot assume this is an ideal gas.

\subsection*{Solution}
\SI{7.97e-4}{\kmol\per\cubic\meter}


\newpage
\section{Molar density of air}

\subsection*{Challenge}
Assuming air to be an ideal gas, calculate the molar density of air, $C_{air}$ at 300 K and atmospheric pressure.

\subsection*{Solution}
\SI{4.1e-2}{\kmol\per\cubic\meter}