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<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">I always get several questions about exp 23. I realize we haven't had<br>
a chance to cover this material yet but will get through some of it before<br>
the reports are due. The following should help lead you in the right<br>
directions.<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman""><o:p> </o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">There’s a Excel file for the Data-to-Collect tables (page 162 in the manual)<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">and report table for Part C (page 163 in the manual) on Carmen.<span style="mso-spacerun:yes">
</span>There’s<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">also a template for the report questions.<br>
<br>
For <b>Part A</b>:<br>
<br>
In the lab you were using the Cu electrode as your cathode and it's<br>
acting as the standard electrode (the electrode in the beaker). Each of<br>
your <b>other </b>electrodes are the anodes. Since the other electrodes</span><span style="mso-fareast-font-family:"Times New Roman""> are<br>
the anodes (oxidation) in the reaction, your <span class="SpellE">E^o</span> values for the cell were<br>
for those electrodes being the half-cell where oxidation takes place (the<br>
oxidation reactions). </span><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">For the table in your report you need to write the<br>
reactions as reduction reactions (which means if you've written them<br>
in the notebook or report as oxidation reactions you will need to reverse<br>
them so they are written as reduction reactions). You should get a table<br>
which looks like Table 20.1 in the textbook (p. 863 in the 14th ed., p. 871<br>
in the 13th ed., p. 841 in the 12th ed., p. 857 in the 11th ed. and p. 863 in<br>
the 10th ed.) and Table 23.1 in the manual (page 151).<br>
<br>
Essentially what you were doing is using the Cu electrode as the<br>
standard electrode rather then the normal standard hydrogen electrode (SHE).<br>
If you look at Table 20.1 you will see the SHE has a value of zero and the Cu<br>
electrode as an <span class="SpellE">E^o</span> of 0.34 V. You could redo Table 20.1 by making the Cu<br>
electrode have a value of 0, which means you would be subtracting 0.34 from<br>
the values in Table 20.1. So if you based the table on a standard Cu electrode<br>
all the values in Table 20.1 would change by 0.34 (decrease by 0.34). In this<br>
"new" table the value for the hydrogen electrode would be -0.34 V.<br>
<br>
Rather than do all this, we are having you use the <span class="SpellE">eqn</span> used in class, the<br>
textbook and manual which relates the <span class="SpellE">E^o</span> for the cell to the
<span class="SpellE">E^o</span> values of<br>
the cathode and anode,<br>
<br>
<span class="SpellE">E^o</span>(cell) = <span class="SpellE">E^o_red</span> (cathode) -
<span class="SpellE">E^o_red</span>(anode),<br>
<br>
as given on page 152 of the manual. Using this <span class="SpellE">eqn</span> with the
<span class="SpellE">E^o_cell</span><br>
which you got in the lab you should get <span class="SpellE">E^o_red</span> (anode) for your anodes which<br>
should agree with those given in Table 20.1 (and Appendix E) of the book. The<br>
<span class="SpellE">E^o_red</span> for Cu should wind up being 0.34, as given in Table 20.1. Your value for<br>
the Fe electrode should wind up being -0.44. You will likely find some of your<br>
values don't agree with those in Table 20.1 (or Appendix E). <br>
</span><span style="mso-fareast-font-family:"Times New Roman""><br>
</span><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">For
<b>Part B</b>:<br>
<br>
This is like Part A. The more conc. soln. of Cu^2+ is the cathode (the dilute <span class="SpellE">
soln</span><br>
is the anode). Compare the values you get with that for a standard electrode<br>
when the conc. of both <span class="SpellE">solns</span> would be 1 M. What's the differences? Why?<br>
Look at the Nernst Eqn. in section 20.6 of the textbook. In this <span class="SpellE">
eqn</span> for a conc.<br>
cell the conc. of the metal cation for the anode (oxidation) is in the numerator and<br>
the conc. of the metal cation for the cathode (reduction) is in the denominator in<br>
the reaction quotient, Q. Calculate what the E for these <span class="SpellE">conc.cells</span> should be and<br>
how do your experimental values compare with the calc. ones.<br>
<br>
<br>
For <b>Part C</b>:<br>
<br>
Your table should look like that on page 163 of the manual (and is in the Excel<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">file).<span style="mso-spacerun:yes">
</span>The 2nd column is "moles of <b>metal </b>calculated from the current". It might<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">make things easier if you add another column for the moles of electrons<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">transferred but it's not necessary.<br>
<br>
The calculated AWs for the two electrodes should be the same since you<br>
are using the same electrodes. The mass gained at the cathode should equal<br>
mass lost by the anode. Since the moles lost by the anode equals the moles<br>
gained at the cathode the AWs should be the same. However, you will find<br>
you may not get the same AWs. <o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman""><br>
Your calculation for the moles of electrons will look similar to that on page<br>
155 of the manual. Use what ever time period you actual had (30.0 min,<br>
30.5 min, 31.0 min etc.) Then you need to calculate the moles of metal<br>
lost at the anode and gained at the cathode. That's part of the calculations<br>
shown on page 156, EXCEPT it's only the first multiplication shown and you<br>
do NOT use the AW to calculate mass. You are just getting the moles of<br>
metal. Since all your metals involve a 2-electron transfer it will look like the<br>
first step for Cu on page 156 (hint: all of the ions you used had charges,<br>
ox. states, of +2). You are stopping with moles of metal and not going all<br>
the way to mass.<br>
<br>
Then you take the mass of metal gained by the cathode (which you measured<br>
in the lab) and divide by the moles of metal you calculated from the moles of<br>
electrons transferred to get the molar mass (atomic wt.). You do the same for<br>
the anode, using the mass lost by the anode, which you measured in the lab.<br>
The Actual AW is from the periodic table.<br>
<br>
In the table for part C you need to calculate % error. You can find this on<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">page F-5 of the manual and at the following link,<br>
</span><span style="mso-fareast-font-family:"Times New Roman""><br>
</span><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman""><a href="http://chemistry.osu.edu/%7Erzellmer/chem1250/lab/App_F_1250_lab_manual.pdf"><b>Treatment of Numerical Data (Error Analysis, sig. fig., slope from a graph)</b></a>
<br>
<br>
You true value in this calculation is the known AW for your metal from the<br>
periodic table.<br style="mso-special-character:line-break">
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<![endif]><o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman""><o:p> </o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">This is a “short” report.<span style="mso-spacerun:yes">
</span>What you need to include is on page 161 of the manual<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman"">and below.<br>
<br>
<b>Report:</b><br>
<br>
• Cover Page<br>
• Page with Purpose and Procedure<br>
• Sample Calculations<br>
o Calculations for the reduction potential (emf) for one electrode other than Cu/Cu<br>
for Part A<br>
o Calculations for the cell potential for one set of concentrations from Part B (Nernst<br>
Equation)<br>
o Calculations for the table in Part C for either anode or cathode<br>
• Tables <br>
Part A - make a table similar to Table 23.1 on page 151. Make sure you write the<br>
reactions as reductions with the proper electrode potentials (calculated as described<br>
above).<br>
Part B - Make a table with the three Cu/Cu reactions, including conc., and the E for<br>
the different concentrations. For example,<br>
<br>
Cu^2+ (<span class="SpellE">aq</span>, conc. of concentrated) ---> Cu^2+ (<span class="SpellE">aq</span>, conc. of dilute) E value<br>
<br>
Cu^2+ (<span class="SpellE">aq</span>, 1.0 M) ----> Cu^2+ (<span class="SpellE">aq</span>, 1.0 M) E value<br>
Cu^2+ (<span class="SpellE">aq</span>, 1.0 M) ----> Cu^2+ (<span class="SpellE">aq</span>, 0.1 M) E value<br>
Cu^2+ (<span class="SpellE">aq</span>, 1.0 M) ----> Cu^2+ (<span class="SpellE">aq</span>, 0.01 M) E value<br>
<br>
Part C - table like that on page 163 (in Excel file)<br>
<br>
• Answers to Questions (explain your answers) - this is the "template" on Carmen.<br>
That's provided so you wouldn't have to type out the questions.<br>
<br>
There is NO Discussion or Conclusion sections for this report.<br>
<br>
</span><b><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman";color:red">The report MUST be typed. NO scans.</span></b><span style="font-size:12.0pt;mso-fareast-font-family:"Times New Roman""><br>
<br>
<br>
<b>Rubric and Sample Calculations:</b><br>
<br>
Look at the PDF rubric given in the module. It makes it a little easier to determine<br>
what's required for the sample calcs.<br>
<br>
The table in part C lists "Moles of Metal". You should show a calculation<br>
for moles of e- transferred and then moles of metal, as shown on the rubric.<br>
If you do it all as one step that's fine (using dimensional analysis you could<br>
do it all in one long step). Remember, you are supposed to show a sample<br>
for every calculation.<br>
<br>
<b>Post Lab:</b><br>
<br>
There's a post-lab on Carmen.<br>
<br>
Dr. Zellmer</span><span style="mso-fareast-font-family:"Times New Roman""> <o:p></o:p></span></p>
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