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<tt><font size="+2">Quiz 1 will cover the following: Chapter 13
(13.1-13.6) and Sections 14.1-14.3 <br>
<br>
This is pretty much up through this past Monday. The only thing
from today's<br>
(Wed.) lecture is section 14.3 (the initial rate problems, we'll
finish the<br>
2nd example tomorrow). For the most part that's how coverage
on quizzes<br>
will be, Wed, Fri of one week and Mon of the next week, with
maybe a small<br>
amount from the 2nd Wed. This quiz covers last week's material,
this past<br>
Monday's and 1 example from section 14.3 from today.<br>
<br>
Section 13.1: <br>
<br>
Understand the solution process and energy diagrams, how
solutions form, <br>
ideal, endothermic and exothermic solution formation and the
importance <br>
of entropy in solution formation. In general, when things mix
there is <br>
an inc. in entropy (disorder) but this is not always the case.
An inc. <br>
in entropy is absolutely necessary for an ideal or endothermic
solution <br>
to form. This is not the case for an exothermic process. An
exothermic <br>
process already tends to be spont. so an inc. in entropy is not
necessary <br>
for this type of solution to form. There are cases in which the
delta(H)_soln <br>
is negative (exothermic) and the entropy decreases (solution is
more ordered) <br>
and the solution forms. Also, understand the role of attractive
forces <br>
between particles in solution formation. <br>
<br>
In the 12th-14th editions the delta(H)_solvation is referred to
as the<br>
the delta(H)_mix. This is step 3 (solute-solvent att. forces
step),<br>
the exothermic step in the solution process as seen in my
figures in the<br>
notes and Figure 13.4. The book doesn't show an ideal solution
figure but<br>
I have it in the notes.<br>
<br>
I also have a link showing the solution enthalpy diagrams
including a <br>
discussion about the attractive forces and entropy, "Ch. 13 -
Solution <br>
Formation and Solubility Effects" in the "Notes" section of the
course web <br>
page. <br>
<br>
</font></tt><tt><font size="+2"><a
href="https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch13_soln_formation.pdf"><b>Ch.
13 - Solution Formation and Solubility Effects</b></a> <br>
<br>
Section 13.2: <br>
<br>
Solubility, saturated, unsaturated and supersaturated solutions.
<br>
<br>
Section 13.3: <br>
<br>
Factors affecting solubility - Att. forces ("like dissolves
like"), pressure <br>
and temp. affects. You're considering temp. effects and "like
dissolves like" <br>
concepts in exp 1 (SOL). <br>
<br>
I have summary on line about attractive forces and solubility.
See the link <br>
below in the "Notes" section of my course web page.<br>
<br>
</font></tt><tt><font size="+2"><a
href="https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch11_12_13_rev.htm"><b>Ch.
11/12 & 13 - Review of IAF, Solids & Solubility</b></a><br>
<br>
<br>
Section 13.4: <br>
<br>
concentration units (know definitions, how to calculate them,
how to use them <br>
as conversion factors in problems and how to convert from one
conc. unit to <br>
another - see my examples in the notes and on the class web page
on the easiest <br>
way to approach these types of problems). <br>
<br>
Sections 13.5-13.6: <br>
<br>
Make sure you can do colligative property calculations,
including<br>
for ionic substances or ionizing molecular substances (things
that<br>
dissociate or ionize to give multiple particles, NaCl, HCl,
etc.).<br>
Know what the van't Hoff factor is (effective # particles or<br>
observed "i" - see "A Closer Look" on page 551, 14th ed., page
558,<br>
13th ed., page 540, 12th ed., 554, 11th ed., page 557, 10th ed.<br>
and my notes). Look at the link I have about colligative
properties<br>
under the "Helpful Tidbits" link,<br>
<br>
</font></tt><tt><font size="+2"><a
href="https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/faq/collig_prop.txt"><b>Colligative
Properties</b></a> <br>
<br>
which was e-mailed earlier. It discusses colligative properties
and<br>
"i" (the van't Hoff factor).<br>
<br>
Understand how osmosis effects cells. <br>
<br>
Finally, you should understand what colloids are and how you
tell <br>
whether you have a colloid or a solution (Tyndall effect).
Also, you <br>
should know the difference between hydrophilic and hydrophobic
colloids. <br>
<br>
You should review Ch 11 material. Review section 2.7-2.8 on
ions, <br>
their charges and polyatomic ions, which stay together as a
single unit<br>
when an ionic compound dissolves. Also, review sections 4.1-4.3
which<br>
deal with electrolytes and nonelectrolytes in solution and
acid/base reactions.<br>
Look at tables 4.2 and 4.3 in relation to strong and weak acids
and bases. <br>
<br>
<b>Homework coverage (you should be able to all problems in the
given ranges)</b><b>:</b><br>
<br>
For those of you using the 14th edition the quiz covers sections
13.1-13.6<br>
You should be able do to homework problems 13.1-13.114<br>
<br>
For those of you using the 13th edition the quiz covers sections
13.1-13.6<br>
You should be able do to homework problems 13.1-13.114<br>
<br>
For those of you using the 12th edition the quiz covers sections
13.1-13.6<br>
You should be able do to homework problems 13.1-13.113<br>
<br>
For those of you using the 11th edition the quiz covers sections
13.1-13.6<br>
You should be able do homework problems 13.1-13.112<br>
<br>
<b>For the on-line homework:</b><b><br>
</b><br>
Do ch 11 tutorial as a review. Do ch 13 homework. Remember
there<br>
are the DSM questions and review problems for Ch 13 (plus a
tutorial<br>
which isn't for credit).<br>
<br>
<br>
Sections 14.1-14.3: <br>
<br>
Know what rate is and how it is related to concentration (rate
law). <br>
Know what a rate law is and how you can use it, what the order
is, rate <br>
constant, etc. Know how reaction rates and stoichiometry are
related and <br>
how the rates of disappearance of reactants and appearance of
products can <br>
be related to each other and the rate of the reaction (using the
balanced <br>
equation). <br>
<br>
Know how to obtain a rate from data and how to use rate data to
determine <br>
the rate law using the method of initial rates. This is shown
in the book <br>
in sample ex 14.6 (and the practice exercise) and my notes. You
really need <br>
to learn how to do this using the second example I used in
lecture (the long <br>
one). If you don't you will have problems with some of the
end-of-chapter <br>
exercises (especially the last one for section 14.3). <br>
<br>
Remember, rate laws can depend on concentration of reactants,
products and <br>
catalysts. The orders of substances in the rate law can be
whole numbers, <br>
simple fractions, negative (usually seen for products and
inhibitors). To <br>
get the overall order you simply add the orders for everything
in the rate <br>
law. Also, remember in general you can't write the rate law
from the balanced <br>
chemical equation. It must be determined experimentally. The
ONLY time you <br>
can write a rate law from a balanced eqn is if you know the
reaction is an <br>
elementary reaction (a single-step mechanism) and you don't know
this by <br>
simply looking at the reaction. <br>
<br>
<b>Homework coverage (you should be able to all problems in the
given ranges)</b><b>:</b><b><br>
</b></font></tt><tt><font size="+2"><b><br>
</b></font></tt><tt><font size="+2">For those of you using the
14th edition the quiz covers sections 14.1-14.3<br>
You should be able do to homework problems </font></tt><tt><font
size="+2">14.1-14.5, 14.17-14.38, <br>
14.89-14.94, 14.117 <br>
<br>
For those of you using the 13th edition the quiz covers sections
14.1-14.3<br>
You should be able do to homework </font></tt><tt><font
size="+2"><font size="+2">problems </font><font size="+2">14.1-14.5,
14.17-14.38, <br>
14.89-14.94, 14.117<br>
<br>
</font> For those of you using the 12th edition the quiz covers
sections 14.1-14.3<br>
You should be able do to homework problems </font></tt><tt><font
size="+2">14.1-14.6, 14.17-14.38,<br>
14.97-14.100, 14.119 <br>
<br>
For those of you using the 11th edition the quiz covers sections
14.1-14.3<br>
You should be able do to homework problems </font></tt><tt><font
size="+2">14.1-14.4, 14.13-14.34,<br>
14.83-14.86, 14.104 <br>
<br>
<b>For the on-line homework:</b><b><br>
</b></font></tt><tt><br>
</tt><tt><font size="+2"><font size="+2">Do ch 14 homework.
Remember there are the DSM questions and review<br>
problems for Ch 14 (plus a tutorial which isn't for credit).<br>
</font> <br>
<br>
Dr. Zellmer </font></tt>
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