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<div class="moz-cite-prefix">On 09/16/2015 05:38 PM, wrote:<br>
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<p>Hi Dr. Pounds!</p>
<p><br>
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<p>MY and I were wondering how to calculate the theoretical
moles of alum. Do we take the theoretical mass of alum and
divide it by the actual mass that we produced? How do we
approach the problem?</p>
<p><br>
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<p>Thank you!</p>
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<br>
It's just like you did on the prelab and like the the theoretical
yield problem I did last week in class.<br>
<br>
What is difficult is following all the equations to determine what
the ratio is between the aluminium and the alum. It is 1 to 1; one
mole of aluminium produces one mole of alum. Compute the moles of
aluminium and then use that to compute the moles of alum. Use the
molar mass of the alum and the moles of alum to then determine your
theoretical yield.<br>
<br>
The percent yield is then the actual yield (what you made) divided
by the theoretical yield with that quantity multiplied by 100 to
give you a percentage instead of a fraction.<br>
<br>
<pre class="moz-signature" cols="72">--
Andrew J. Pounds, Ph.D.
Professor of Chemistry and Computer Science
Mercer University, Macon, GA 31207 (478) 301-5627
<a class="moz-txt-link-freetext" href="http://faculty.mercer.edu/pounds_aj">http://faculty.mercer.edu/pounds_aj</a>
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