\documentclass[11pt]{article}
\pagestyle{empty}

\parindent=0pt
\parskip=.1in

\begin{document}


\centerline{\textbf{Temperature change of dissolving salt}}
\bigskip

Given that the enthalpy of dissolution (dissolving) of NaCl in water is
  $4\times 10^3$ J/mol and the specific heat $c_p$ of water is
  4.2~J/g$\cdot$K, what is the change in temperature of a cup holding
  100~g of water (moderately well insulated), if you dissolve 30~g of
  salt in it?
  
\bigskip

After you have found the change in temperature, discuss the following questions with your group:

\begin{itemize}
\item What happened to the entropy of the isolated salt plus water system?
\item  Can we predict the value of the entropy change from the information
  given? 
\item Could we \emph{measure} the change in entropy? How?
\item   What assumptions did we make when performing this calculation?
\item  \emph{Can we do this experiment?}
\end{itemize}

\vfill
\leftline{\textit{by David Roundy}}
\leftline{\copyright DATE David Roundy}

\end{document}