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<tt>Quiz 2 will cover the following: </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Chapter 14 (14.4-14.7), Chapter 15 (15.1-15.7) </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt>There is some overlap with quiz 1 for chapter 14 (as in
knowing</tt><tt><br>
</tt><tt>what a rate law is - Section 14.3).</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> <b>Section 14.3: </b></tt><tt><br>
</tt><tt><br>
</tt><tt>Technically this section was on the first quiz and while
you might</tt><tt><br>
</tt><tt>not be directly quizzed on this stuff you still need to
know these things.</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know how to obtain a rate from data and how to use rate
data to determine</tt><tt><br>
</tt><tt>the rate law using the method of initial rates. This is
shown in the book</tt><tt><br>
</tt><tt>in sample ex 14.6 (and the practice exercise) and my
notes. You really need</tt><tt><br>
</tt><tt>to learn how to do this using the second example I used in
lecture (the long</tt><tt><br>
</tt><tt>one). If you don't you will have problems with some of the
end-of-chapter</tt><tt><br>
</tt><tt>exercises (especially the last one for section 14.3).</tt><tt>
</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Remember, rate laws can depend on concentration of
reactants, products and</tt><tt><br>
</tt><tt>catalysts. The orders of substances in the rate law can be
whole numbers,</tt><tt><br>
</tt><tt>simple fractions, negative (usually seen for products and
inhibitors). To</tt><tt><br>
</tt><tt>get the overall order you simply add the orders for
everything in the rate</tt><tt><br>
</tt><tt>law. Also, remember in general you can't write the rate
law from the balanced</tt><tt><br>
</tt><tt>chemical equation. It must be determined experimentally.
The ONLY time you</tt><tt><br>
</tt><tt>can write a rate law from a balanced eqn is if you know the
reaction is an</tt><tt><br>
</tt><tt>elementary reaction (a single-step mechanism) and you don't
know this by</tt><tt><br>
</tt><tt>simply looking at the reaction.</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> <b>Section 14.4:</b> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know what an integrated rate equation is for zero-order,
1st-order and</tt><tt><br>
</tt><tt>2nd-order reactions and be able to use them. Know what the
half-life is</tt><tt><br>
</tt><tt>for zero-order, 1st-order and 2nd-order reactions. This is
in section 14.4.</tt><tt><br>
</tt><tt>The equations for zero-order are in the notes. There are a
couple of</tt><tt><br>
</tt><tt>questions in the chapter 14 "handouts" about zero and 2nd
order reactions</tt><tt><br>
</tt><tt>on my class web page (see "Notes" link). Be able to do the
special problem</tt><tt><br>
</tt><tt>passed out in class and sent via e-mail. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> <b>Section 14.5: </b></tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Understand the relationship between temp., activation
energy (Ea) and rate </tt><tt><br>
</tt><tt> constant (Arrhenius eqn.) and the rate of the reaction.
Understand how all </tt><tt><br>
</tt><tt> this relates to collision theory and transition state
theory. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> <b>Section 14.6: </b></tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Understand mechanisms and how to obtain a rate law from a
mechanism, </tt><tt><br>
</tt><tt> rate laws for elementary reactions, recognize
intermediates, </tt><tt><br>
</tt><tt> and what molecularity means. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Remember, steps in a mechanism are always written as
elementary processes, </tt><tt><br>
</tt><tt> which means the rate law for a step can be written from
the balanced eqn </tt><tt><br>
</tt><tt> for that step. This is the ONLY time you can write the
rate law from a </tt><tt><br>
</tt><tt> balanced eqn. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> <b>Section 14.7: </b></tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know what catalysts are and the four common
characteristics of catalysts, </tt><tt><br>
</tt><tt> homogeneous and heterogeneous catalysis, how catalysts
work and be able </tt><tt><br>
</tt><tt> to recognize a substance as a catalyst or intermediate in
a mechanism. Know </tt><tt><br>
</tt><tt> how a catalyst affects rate and how this can be seen using
the Arrhenius eqn. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> You can find the handouts mentioned above at </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><a
href="http://www.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch14houts.pdf"><b>Chapter
14 - Chemical Kinetics - Handouts</b> </a></tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt><br>
<b>Homework coverage (you should be able to all problems in the
given ranges):</b></tt><tt><br>
</tt><tt><br>
</tt><tt>For those of you using the 14th edition the quiz covers
sections 14.1-14.4</tt><tt><br>
</tt><tt>You should be able to do homework problems 14.1-14.8,
14.17-14.50,</tt><tt><br>
</tt><tt>14.89-14.103, 14.117</tt><tt><br>
</tt><tt><br>
</tt><tt>For those of you using the 13th edition the quiz covers
sections 14.1-14.4</tt><tt><br>
</tt><tt>You should be able to do homework problems 14.1-14.8,
14.17-14.50,</tt><tt><br>
</tt><tt>14.89-14.103, 14.117</tt><tt><br>
</tt><tt><br>
</tt><tt>For those of you using the 12th edition the quiz covers
sections 14.1-14.4</tt><tt><br>
</tt><tt>You should be able to do homework problems 14.1-14.8,
14.17-14.52,</tt><tt><br>
</tt><tt>14.97-14.109, 14.119</tt><tt><br>
</tt><tt><br>
</tt><tt>For those of you using the 11th edition the quiz covers
sections 14.1-14.4</tt><tt><br>
</tt><tt>You should be able to do homework problems 14.1-14.6,
14.13-14.46,</tt><tt><br>
</tt><tt>14.83-14.93, 14.104</tt><tt><br>
</tt><tt><br>
</tt><b><tt>For the on-line homework:</tt></b><tt><br>
</tt><tt><br>
</tt><tt>Do ch 14 (14.4-14.7) homework review. Remember there are
the DSM questions</tt><tt><br>
</tt><tt>and review problems for Ch 14 (plus a tutorial which isn't
for credit).</tt><tt><br>
</tt><tt><br>
</tt><tt>Don't forget the extra homework problems "handout". They
can also be found</tt><tt><br>
</tt><tt>on my web page at the Notes link (see above) or Homework
link where you will</tt><tt><br>
</tt><tt>also find the solutions,</tt><tt><br>
</tt><tt><br>
</tt><tt> </tt><tt><a
href="http://www.chemistry.ohio-state.edu/%7Erzellmer/chem1220/homewk/ch14hmwk_add.pdf"><b>CH
14 - Kinetics, Extra Problems and Solutions</b></a></tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt><b>You will get the integrated rate equations and half-life
eqns. on the quiz.</b></tt><tt><b><br>
</b></tt><tt><b>They will not be in any particular order nor will
the half-life eqns</b></tt><tt><b><br>
</b></tt><tt><b>necessarily be in the same order as the integrated
rate equations.</b></tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><b><tt>Sections 15.1-15.5: </tt></b><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> You need to understand how to set up an expression for the
equilibrium</tt><tt><br>
</tt><tt>constant, K and how to use it. Understand how to set up K
for heterogeneous</tt><tt><br>
</tt><tt>equilibria (when you have pure solids and liquids involved
in the equilibrium).</tt><tt><br>
</tt><tt>What substances appear in the equilibrium constant
expression? Gases and solutes</tt><tt><br>
</tt><tt>in solution but not pure solids or liquids. How do you
know if something is a</tt><tt><br>
</tt><tt>pure solid or liquid? If there's and (s) or (l) for the
state symbol in the</tt><tt><br>
</tt><tt>balanced equation.</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> What does the magnitude of K tell you? Does the reaction
go to completion </tt><tt><br>
</tt><tt> and by how much (mostly products or "essentially only"
products)? Does the </tt><tt><br>
</tt><tt> reaction "not occur to any great extent" and how little
reaction occurs </tt><tt><br>
</tt><tt> (mostly reactants or "essentially only" reactants)? Are
there appreciable </tt><tt><br>
</tt><tt> amounts of reactants and products at equilibrium? </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Remember K depends on the form of the balanced equation
and you can </tt><tt><br>
</tt><tt> relate the K for one form of the balanced equation to
another. When you</tt><tt><br>
</tt><tt>multiply and eqn by some factor the K for the new reaction
equals the old</tt><tt><br>
</tt><tt>K RAISED to that factor (you do NOT multiply the K by that
factor).</tt><tt><br>
</tt><tt>(e.g. K_rev = 1/K_for or K_for</tt><tt><sup
class="moz-txt-sup"><span
style="display:inline-block;width:0;height:0;overflow:hidden">^</span>-1</sup></tt><tt>
which makes sense since to get the reverse</tt><tt><br>
</tt><tt>rxn you are essentially multiplying the forward rxn by -1).
</tt><tt><br>
</tt><tt> Know the relationship between equilibrium constants when
you add several</tt><tt><br>
</tt><tt>balanced equations to get a new balanced equation (the K's
of the eqns</tt><tt><br>
</tt><tt>being added are multiplied together to get the K for the
resulting new rxn).</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know how to use an equilibrium (ICE) table and use it to
determine K from </tt><tt><br>
</tt><tt> equilibrium concentrations. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know how to relate Kp and Kc. </tt><tt><br>
</tt><tt> </tt><tt><br>
<b>Section 15.6: Applications of Equilibrium Constants</b><br>
<br>
</tt><tt> Understand the reaction quotient, Q, and how you use it
with K to predict </tt><tt><br>
</tt><tt> whether the reaction is at equilibrium or not and if not
which direction </tt><tt><br>
</tt><tt> does it proceed to reach equilibrium. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know how to use an ICE table to calculate equilibrium
conc. starting with </tt><tt><br>
</tt><tt> initial conc. and the equilibrium constant, K. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> On the quiz, if you need to use an ICE table, you MUST
SHOW the WORK</tt><tt><br>
</tt><tt>and the ICE table. When making any assumptions you should
show that your </tt><tt><br>
</tt><tt> assumptions are okay (less than 5% error). If the percent
error is greater </tt><tt><br>
</tt><tt> than 5%, you need to solve the problem in a more exacting
way (solve a </tt><tt><br>
</tt><tt> quadratic, method of successive approximations, etc.).
You must show this</tt><tt><br>
</tt><tt>work. If you don't, you will not get full credit.</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> <b>Section 15.7: Le Chatelier's Principle</b> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Understand how changing conc. shifts a reaction </tt><tt><br>
</tt><tt> (AWAY from ADDED, TOWARD REMOVED). Remember adding or</tt><tt><br>
</tt><tt> removing (small amounts, but not all) of a pure solid or
pure liquid will</tt><tt><br>
</tt><tt> not shift a reaction. Removing all of a pure solid or
pure liquid will shift the </tt><tt><br>
</tt><tt> reaction (toward the removed substance - you have to have
some of the </tt><tt><br>
</tt><tt> solid or liquid to be at equilibrium when they are present
in the rxn). </tt><tt><br>
</tt><tt> Adding or removing a pure liquid which is also the solvent
will cause a</tt><tt><br>
</tt><tt>shift due to an indirect effect (e.g. adding solvent
decreases the conc.</tt><tt><br>
</tt><tt>of the solutes causing the reaction to shift toward more
moles in solution,</tt><tt><br>
</tt><tt>similar to what happens for gases when the pressure
decreases due to a</tt><tt><br>
</tt><tt>volume inc.). I discussed this in relation to exp 19 in
class.</tt><tt><br>
</tt><tt>Conc. changes do NOT affect the numerical value of K. </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Know how changing pressure (due to volume changes) effects
a reaction.</tt><tt><br>
</tt><tt>Increasing pressure (by reducing the volume) shifts the
reaction toward</tt><tt><br>
</tt><tt>fewer moles of gas. Decreasing pressure (by inc. the
volume) shifts</tt><tt><br>
</tt><tt>the reaction toward more moles of gas. Changing volume for
a gas is</tt><tt><br>
</tt><tt>essentially changing the concentration of the gases.
Decreasing volume</tt><tt><br>
</tt><tt>increases the conc. of the gases and shifts the reaction to
the side</tt><tt><br>
</tt><tt>with fewer moles in solution (remember, a gas mixture is a
solution).</tt><tt><br>
</tt><tt>Pressure changes do NOT affect the numerical value of K. </tt><tt><br>
</tt><tt><br>
</tt><tt>Remember, adding an inert (non-reacting) gas to a reaction
involving</tt><tt><br>
</tt><tt>gases will increase the total pressure but will NOT cause a
shift in</tt><tt><br>
</tt><tt>the reaction because the partial pressures of the gases
involved in</tt><tt><br>
</tt><tt>the reaction do not change.</tt><tt><br>
</tt><tt><br>
</tt><tt>Something similar also occurs in reactions taking place in
a liquid solution</tt><tt><br>
</tt><tt>environment. When the volume of solution changes the
reaction will shift</tt><tt><br>
</tt><tt>if there is a change in moles of dissolved solutes. If the
volume is</tt><tt><br>
</tt><tt>increased by adding solvent the reaction will shift toward
more moles</tt><tt><br>
</tt><tt>of solutes. This is like decreasing pressure by inc.
volume for gases,</tt><tt><br>
</tt><tt>the reaction shifts toward more moles of gas.</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt>Also, know how changing temperature shifts a reaction AND
changes the numerical</tt><tt><br>
</tt><tt>value of the equilibrium constant, K (changing conc. and
pressures do not affect</tt><tt><br>
</tt><tt>the numerical value of K). How does the change in the
forward and reverse rate</tt><tt><br>
</tt><tt>constants (rates) cause the shift in the equilibrium and
affect K for both</tt><tt><br>
</tt><tt>exothermic and endothermic reactions for elementary
reactions? Remember,</tt><tt><br>
</tt><tt>temperature changes have a bigger affect on reactions with
bigger Ea.</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><b><tt>Homework coverage (you should be able to all problems in
the given ranges):</tt></b><b><tt><br>
</tt></b><tt><br>
</tt><tt>For those of you using the 11th - 14th editions the quiz
covers ch 15.</tt><tt><br>
</tt><tt>You should be able to do all homework problems in ch 15.</tt><tt><br>
</tt><tt><br>
</tt><b><tt>For the on-line homework:</tt></b><tt><br>
</tt><tt><br>
</tt><tt>Do ch 15 (15.1-15.7) homework review. Remember there are
the DSM questions</tt><tt><br>
</tt><tt>and review problems for Ch 15 (plus a tutorial which isn't
for credit).</tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Don't forget the extra homework problems. They can be
found on the web at </tt><tt><br>
</tt><tt> the Homework link on the class web page (CH 15 - Extra ICE
Table Problems and </tt><tt><br>
</tt><tt> Solutions), </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><a
href="http://www.chemistry.ohio-state.edu/%7Erzellmer/chem1220/homewk/ch15_extra_problems.pdf"><b>CH
15 - Extra ICE Table Problems and Solutions</b> </a></tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> </tt><tt><br>
</tt><tt> Dr. Zellmer </tt>
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