Quiz 2 material

[zellmer.1]

Quiz 2 will cover the following:  Chapter 13 (13.1-13.6) and Sections 14.1-14.4

Section 13.1:

Understand the solution process and energy diagrams, how solutions form,
ideal, endothermic and exothermic solution formation and the importance
of entropy in solution formation.  In general, when things mix there is
an inc. in entropy (disorder) but this is not always the case.  An inc.
in entropy is absolutely necessary for an ideal or endothermic solution
to form.  This is not the case for an exothermic process.  An exothermic
process already tends to be spont. so an inc. in entropy is not necessary
for this type of solution to form.  There are cases in which the delta(H)_soln
is negative (exothermic) and the entropy decreases (solution is more ordered)
and the solution forms.  Also, understand the role of attractive forces
between particles in solution formation.

In the 12th edition the delta(H)_solvation is referred to as the
the delta(H)_mix.

I also have a link showing the solution enthalpy diagrams including a
discussion about the attractive forces and entropy, "Ch. 13 - Solution
Formation and Solubility Effects" in the "Notes" section of the course web
page.

http://chemistry.osu.edu/~rzellmer/chem1220/notes/ch13_soln_formation.pdf

Section 13.2:

Solubility, saturated, unsaturated and supersaturated solutions.

Section 13.3:

Factors affecting solubility - Att. forces ("like dissolves like"), pressure
and temp. affects. You're considering temp. effects and "like dissolves like"
concepts in exp 15.

I have summary on line about attractive forces and solubility. See the link
"Ch. 11 & 13 - Review of IAF, Solids and Solubility" in the "notes" section of
the course web page.

http://chemistry.osu.edu/~rzellmer/chem1220/notes/ch11_12_13_rev.htm

Section 13.4:

concentration units (know definitions, how to calculate them, how to use them
as conversion factors in problems and how to convert from one conc. unit to
another - see my examples in the notes and on the class web page on the easiest
way to approach these types of problems).

Sections 13.5-13.6:

Make sure you can do colligative property calculations, including
for ionic substances or ionizing molecular substances (things that
dissociate or ionize to give multiple particles, NaCl, HCl, etc.).
Know what the van't Hoff factor is (effective # particles or
observed "i" - see "A Closer Look" on page 540, 12th ed.,
554, 11th ed., page 557, 10th ed. and my notes).  Look at the
link I have about colligative properties under the "Helpful Tidbits"
link,

http://chemistry.osu.edu/~rzellmer/chem1220/faq/collig_prop.txt

which was e-mailed earlier.

Understand how osmosis effects cells.

Finally, you should understand what colloids are and how you tell
whether you have a colloid or a solution (Tyndall effect).  Also, you
should know the difference between hydrophilic and hydrophobic colloids.

You should review section 2.7-2.8 on ions,
their charges and polyatomic ions, which stay together as a
single unit when an ionic compound dissolves.  Also, review sections
4.1-4.3 which deal with electrolytes and nonelectrolytes in solution
and acid/base reactions.  Look at tables 4.2 and 4.3 in relation to
strong and weak acids and bases.

You should be able do to homework problems 13.1-13.112

If you are using the 11th edition do homework problems 13.1-13.112

If you are using the 10th edition do homework problems 13.1-13.107



Sections 14.1-14.3:

Know what rate is and how it is related to concentration (rate law).
Know what a rate law is and how you can use it, what the order is, rate
constant, etc.  Know how reaction rates and stoichiometry are related and
how the rates of disappearance of reactants and appearance of products can
be realted to each other and the rate of the reaction (using the balanced
equation).

Know how to obtain a rate from data and how to use rate data to determine
the rate law using the method of initial rates.  This is shown in the book
in sample ex 14.6 (and the practice exercise) and my notes.  You really need
to learn how to do this using the second example I used in lecture (the long
one).  If you don't you will have problems with some of the end-of-chapter
exercises (especially the last one for section 14.3).

Remember, rate laws can depend on concentration of reactants, products and
catalysts.  The orders of substances in the rate law can be whole numbers,
simple fractions, negative (usually seen for products and inhibitors).  To
get the overall order you simply add the orders for everything in the rate
law.  Also, remember in general you can't write the rate law from the balanced
chemical equation.  It must be determined experimentally.  The ONLY time you
can write a rate law from a balanced eqn is if you know the reaction is an
elementary reaction (a single-step mechanism) and you don't know this by
simply looking at the reaction.

Section 14.4

Know what an integrated rate equation is for zero-order, 1st-order and 2nd-order
reactions and be able to use them.  Know what the half-life is for zero-order,
1st-order and 2nd-order reactions.  This is in section 14.4.  The equations
for zero-order are in the notes and there are a couple of questions in the
chapter 14 handouts passed out in class and on the web (see "notes" link)
about zero and 2nd order.  Be able to do the special problem passed out in
class and sent via e-mail.

You can find the handouts mentioned above
(Chapter 14 - Chemical Kinetics - Handouts) at

http://www.chemistry.ohio-state.edu/~rzellmer/chem122/notes/ch14houts.pdf


You should be able do to homework problems 14.1-14.8, 14.17-14.52,
14.97-14.109, 14.119

For those of you using the 11th edition the quiz covers sections 14.1-14.4
and homework problems 14.1-14.6, 14.13-14.46, 14.83-14.93, 14.104

For those of you using the 10th edition the quiz covers sections 14.1-14.4
and homework problems 14.1-14.5, 14.11-14.44, 14.81-14.89, 14.98


Don't forget the extra homework problems handed out in class.  They can also
be found on the web at the Notes link (see above) or Homework link where you
will also find the solutions (CH 14 - Kinetics, Extra Problems and Solutions),

http://www.chemistry.ohio-state.edu/~rzellmer/chem122/homewk/122ch14hmwk_add.pdf


You will get the integrated rate equations and half-life eqns. on the quiz.
They will not be in any particular order nor will the half-life eqns
necessarily be in the same order as the integrated rate equations.


Dr. Zellmer