|
|
| Goal
I. Know the vocabulary and basic concepts of thermochemistry that describe
and explain energy changes accompanying chemical reactions. |
Objectives: To meet the requirements of Goal
I, you must be able to:
-
differentiate
between
system
and surroundings, between potential energy and kinetic
energy, between spontaneous
and non-spontaneuous changes,
between exothermic and endothermic processes;
-
describe the
sign (+ or -) conventions for heat, work, and thermal energy
(q);
-
describe
how reaction spontaneity is governed by the thermal energy changes and
the entropy changes within the system;
-
convert among
the units: calorie, kilocalorie, joule and kilojoule;
-
distinguish between
specific
heat and heat capacity;
-
use
equations: thermal
energy = (mass)(specific heat)(temp); thermal
energy change = (heat capacity)(temp. change)to calculate
any variable, given appropriate data. [Top]
| Goal II. Apply the principles
of thermochemistry to calorimetric data collection and calculations. |
Objectives: To meet the requirements of Goal
II, you must be able to:
-
explain the experimental
procedure of calorimetry, and describe a simple constant pressure
calorimeter (coffee cup calorimeter);
-
apply
the law of conservation of energy to thermal energy changes taking
place in a calorimeter;
-
calculate
the heat capacity of a calorimeter (also called calorimeter constant)
from mass and temperature data;
-
use
calorimetry data to calculate specific heat, Dt,
final temperature, heat of neutralization or heat of solution. [Top]
| Goal III. Use Hess's Law
and heats of formation to calculate enthalpy changes during a chemical
reaction. |
Objectives: To meet the requirements of Goal
III, you must be able to:
-
relate enthalpy
change (DH)
to thermal energy change at constant pressure; identify
exothermic
and endothermic reactions from thermochemical equations;
-
recognize DH
to be an extensive property; use a thermochemical equation to determine
DH
for a specified amount of reactant or product;
-
state Hess's
Law and relate this law to changes in a state function such as enthalpy;
use this law to determine DHrxn
by combining thermochemical equations;
-
define the
standard heat of formation (DH°¦),a
nd know the standard conditions for thermochemical reactions;
-
write appropriatechemical
equations for specific examples of DHrxn
including DHcomb,
DHvap,
DHfus, DHneut
and DH°¦;
-
calculate enthalpies
of reaction from enthalpies of formation;
and calculate enthalpies of formation
from enthalpies of reaction. [Top]
|
Unit 6 Assignments
|
| Read: |
Text
Chapter 6, pp. 224-251 |
| Video
Programs: |
- Energy
- Enthalpy Changes
and Calorimetry
- Heats of Reaction,
Hess's Law
|
| Textbook
Assignments: |
Read
and Understand all "Sample Problems," "Follow
Up Problems" and the blue-colored problems at the
end of the chapters.
The
answers for the Follow Up Problems are at the end
of the chapter; the answers for the blue-colored
problems are in Appendix C.The answers for each
of these are in Appendix C.
|
| ChemSkill
Builder Assignments: |
Mandatory
assignments to be submitted for grade
Chapter 8, Sections
8.1, 8.2, 8.3, 8.4, 8.5, 8.6
|
| Do Cyber Lab 6: |
See CHM 111 Laboratory Guide. Submit via mail to ELI. |
| TAKE
EXAM 3: |
Exam 3 Covers
Units 5 and 6. You will be given a periodic table
(without the names of the elements). All necessary
heats of formation are also given.
You may use a 3" x 5" hand-written study card for Exams 1, 2, 3, 4, and 5. (NOT TO BE USED FOR THE NOMENCLATURE TEST.) You must hand-write the information you would like to have on your card yourself -- no technology miracles allowed. Formulas, constants, definitions, concepts, solubility tables, etc., may be on the study card. NO SAMPLE PROBLEMS are allowed to be on the card. You may write on both sides of the study card. The card must be submitted with your exam. Any abuse of this privilege will result in a failing grade for the course. ) |
| Note:
Complete Solutions, including all units of measurement,
must be shown for all problems. |
[Top]
|
