<html>
<head>
<title>Lecture 12/4/96, Chapter 12, Section 1-2</title>
</head>
<h1>Lecture 12/4/96, Chapter 12, Section 1-2</h1>
<H2>Announcements</H2>
<B>Assignment: Due Monday, 12/9/96 5:00 pm</B><BR><A HREF="http://science.widener.edu/svb/homework/gaslaw.html">Chapter 12 Homework Set</A> and <BR>
Questions: 11, 15, 17, 19, 27, 29, 33, 35, 39, 45, 49, 53, 59, 73, 83, 111, 119.<P>
<H2>Introduction to Gas Laws</H2>
Solutions to Lecture Problems (<A HREF="lm_c12_a.pdf">pdf</A>, <A
HREF="lm_c12_a.rpl">rpl</A>)<P>
Gas Law Spreadsheet (<A HREF="gaslaw.wk4">Lotus</A>, <A HREF="gaslaw.xls">Excel</A>)
<P>
<ol>
<li>Measurments</li>
<ol>
<li>Pressure (what it is and units)</li>
<Table border>
<TR><TD>Pa</TD> <TD>(N/m<sup>2</sup>)</TD> <TD>101325 Pa = 1 atm</TD></TR>
<TR><TD>bar</TD> <TD>(10<sup>5</sup> Pa)</TD> <TD>1.01325 bar = 1 atm</TR>
<TR><TD>torr and mmHg</TD> <TD>(133.322 Pa)</TD> <TD>760 torr = 1 atm</TR>
<TR><TD>atmosphere</TD> <TD>(101325 Pa)</TD><TD></TD></TR>
<TR><TD>PSI</TD> <TD>(6894.76 Pa)</TD> <TD> 14.7 PSI = 1 atm</TD></TR>
</table><P>
<li>Temperature (Use Kelvin Scale, 273.15)</li><P>
<li>Volume conversions</li>
<TABLE BORDER=1>
<TR>
<TD>Unit</TD>
<TD>Liter</TD>
<TD>m<SUP>3</SUP></TD>
</TR>
<TR>
<TD>m<SUP>3</SUP></TD>
<TD>10<SUP>-3</SUP> </TD>
<TD>1 </TD>
</TR>
<TR>
<TD>cm<SUP>3</SUP> (ml)</TD>
<TD>10<SUP>3</SUP> </TD>
<TD>10<SUP>6</SUP> </TD>
</TR>
<TR>
<TD>liter (dm<SUP>3</SUP>)</TD>
<TD>1 </TD>
<TD>10<SUP>3</SUP> </TD>
</TR>
<TR>
<TD>ft<SUP>3</SUP></TD>
<TD>0.02831 </TD>
<TD>28.31 </TD>
</TR>
<TR>
<TD>in<SUP>3</SUP></TD>
<TD>1.639 x 10<SUP>-5</SUP> </TD>
<TD>0.01639 </TD>
</TR>
</TABLE><P>
</ol>
<li>Introduce concept of an ideal gas</li>
<ol type=a>
<li>No volume</li>
<li>No interaction</li>
<li>Discuss behavior of ideal gas</li></OL><P>
<li>Standard Temperature and Pressure (STP)</li>
<ol type=a>
<li>1 bar (10<SUP>5</SUP> Pa), previously 1 atm</li>
<li>0 °C</li>
</ol><P>
<li>Boyle's Law (PV = C<SUB>B</SUB>)</li>
<ol type=a>
<li>Derive relationship from ideal gas concept with picture on board</li>
<LI>Animation from CD-ROM (
<A HREF="file:///D|/CHAPTERS/MEDIA/CH12_MED/12m10an3.mov">d:</A>,
<A HREF="file:///E|/CHAPTERS/MEDIA/CH12_MED/12m10an3.mov">e:</A>,
<A HREF="file:///F|/CHAPTERS/MEDIA/CH12_MED/12m10an3.mov">f:</A>,
<A HREF="file:///G|/CHAPTERS/MEDIA/CH12_MED/12m10an3.mov">g:</A>,
<A HREF="file:///h|/CHAPTERS/MEDIA/CH12_MED/12m10an3.mov">h:</A>
)
<li>Graph relationship</li>
<li>Write equation for graph</li>
<li>Work a problem. Given an initial volume of 350 in<sup>3</sup> and a compression ratio of 10:1,
what is the final volume?</li>
</ol><P>
<li>P/T = C</li>
<ol type=a>
<li>Derive relationship from ideal gas concept with picture on board</li>
<LI>Animation from CD-ROM (
<A HREF="file:///D|/CHAPTERS/MEDIA/CH12_MED/12m10an2.mov">d:</A>,
<A HREF="file:///E|/CHAPTERS/MEDIA/CH12_MED/12m10an2.mov">e:</A>,
<A HREF="file:///F|/CHAPTERS/MEDIA/CH12_MED/12m10an2.mov">f:</A>,
<A HREF="file:///G|/CHAPTERS/MEDIA/CH12_MED/12m10an2.mov">g:</A>,
<A HREF="file:///h|/CHAPTERS/MEDIA/CH12_MED/12m10an2.mov">h:</A>
)
<li>Graph relationship</li>
<li>Write equation for graph</li>
<li>Work a problem. A pressure cooker starts out at 25 C and 1 atm pressure. What is
the pressure at 200 C?</li>
</ol><P>
<li>Charles Law (V/T = C<SUB>C</SUB>)</li>
<ol type=a>
<li>Derive relationship from ideal gas concept with picture on board</li>
<li>Graph relationship</li>
<li>Write equation for graph</li>
<li>Work a problem. 1 m<sup>3</sup> of steam is heated from 100 C to 500 C at constant pressure.
What is the final volume?</li>
</ol><P>
<li>P/n = C</li>
<ol type=a>
<li>Derive relationship from ideal gas concept with picture on board</li>
<LI>Animation from CD-ROM (
<A HREF="file:///D|/CHAPTERS/MEDIA/CH12_MED/12m10an1.mov">d:</A>,
<A HREF="file:///E|/CHAPTERS/MEDIA/CH12_MED/12m10an1.mov">e:</A>,
<A HREF="file:///F|/CHAPTERS/MEDIA/CH12_MED/12m10an1.mov">f:</A>,
<A HREF="file:///G|/CHAPTERS/MEDIA/CH12_MED/12m10an1.mov">g:</A>,
<A HREF="file:///h|/CHAPTERS/MEDIA/CH12_MED/12m10an1.mov">h:</A>
)
<li>Graph relationship</li>
<li>Write equation for graph</li>
<li>Work a problem. </li>
</ol><P>
<li>Combine above equations to get (PV)/T = C</li><P>
<IMG SRC="ch12_eq_a1.gif" WIDTH=781 HEIGHT=84>
<li>Practice Problems.
<OL Type=a>
<LI>A stratospheric sampling balloon starts at sea level, 760 torr and 20 C with
a volume of 1000 m<sup>3</sup>. The balloon rises to a pressure altitude of 1000 Pa (appx 40
km) where the temperature is -40 C. What is the volume of the balloon at this altitude?</li><P>
<li>Gas data for 1 gram at STP. Calculate the molar volume</li>
<ol>
<li>H<sub>2</sub> 11.1 L</li>
<li>He 5.57 L</li>
<li>N<sub>2</sub> 0.800 L</li>
<li>Cl<sub>2</sub> 0.316 L</li>
</ol></OL></OL>
<p><hr>
<H2><A HREF="../index.html#introduction to gas laws">Return to Paper</A></H2>
<HR>
<p>This page is maintained by <br>
<a href="http://science.widener.edu/~svanbram">Scott Van Bramer</a><br>
<a href="http://www.widener.edu/CAS/chemistry">Department of Chemistry</a><br>
<a href="http://www.widener.edu">Widener University</a><br>
Chester, PA 19013
<p>Please send any comments, corrections, or suggestions to <a
href="mailto:svanbram@science.widener.edu">svanbram@science.widener.edu</a>.
<p>This page has been accessed <!--#exec cgi="/cgi-bin/counter"--> times since 3/23/97 .<br>
Last Updated 3/23/97
</body>
</html>