Download CHS CHEM Ch6Syl ThermoChemistry2016

UNIT 2: Chapter 6: Thermochemistry
DATE(S)
11/2
11/2
11/2
11/7
11/8
11/9, 16
TOPIC AND OBJECTIVE
6.1 Energy and Its Units
 Define energy, kinetic energy,
potential energy, and internal energy.
 Define the SI unit of energy joule, as
well as the common unit of energy
calorie.
 Calculate the kinetic energy of a
moving object. (Example 6.1)
 State the law of conservation of
energy.
6.2 Heat of Reaction
 Define a thermodynamic system and
its surroundings.
 Define heat and heat of reaction.
 Distinguish between an exothermic
process and an endothermic process.
6.3 Enthalpy and Enthalpy Change
 Define enthalpy and enthalpy of
reaction.
 Explain how the terms enthalpy of
reaction and heat of reaction are
related.
 Explain how enthalpy and internal
energy are related.
6.4 Thermochemical Equations
 Define a thermochemical equation.
 Write a thermochemical equation
given pertinent information.
(Example 6.2)
 Learn the two rules for manipulating
(reversing and multiplying)
thermochemical equations.
 Manipulate a thermochemical
equation using these rules. (Example
6.3)
6.5 Applying Stoichiometry to Heats of
Reaction
 Calculate the heat absorbed or
evolved from a reaction given its
enthalpy of reaction and the mass of
a reactant or product. (Example 6.4)
6.6 Measuring Heats of Reaction
 Define heat capacity and specific
heat.
 Relate the heat absorbed or evolved
to the specific heat, mass, and
temperature change.
 Calculate using this relation between
heat and specific heat. (Example 6.5)
 Define calorimeter.
 Calculate the enthalpy of reaction
from calorimetric data (its
temperature change and heat
capacity). (Example 6.6)
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PAGE(S)
Reading
Assignment
Pg225-228
HOMEWORK
Assigned Problems:
#42, 87, 88, 89 90
Recommended additional problems:
4,6
Pg228-231
Assigned Problem:
27
Pg231-234
Assigned Problem:
# 30
Recommended additional problems
7, 8
Pg234-237
Recommended additional problems
#10, 11, 53, 54, 56,
Pg237-238
Assigned Problems:
# 59, 60
Recommended additional problem:
12!
Pg238-242
Assigned Problems:
# 65, 66, 67,68, 69, 70, 101, 102, 103,
104, 105, 106, 107, 108,
Recommended additional problems:
14, 28, 29, 34, 64, 67!, 97!
UNIT 2: Chapter 6: Thermochemistry
11/17, 18
11/22, 23
11/29, 30 &
12/1
12/2
CHS CHEMISTRY
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6.7 Hess’s Law
 State Hess’s law of heat summation.
 Apply Hess’s law to obtain the
enthalpy change for one reaction
from the enthalpy changes of a
number of other reactions. (Example
6.7)
6.8 Standard Enthalpies of Formation
 Define standard state and reference
form.
 Define standard enthalpy of
formation.
 Calculate the heat of a phase
transition using standard enthalpies
of formation for the different phases.
(Example 6.8)
 Calculate the heat (enthalpy) of
reaction from the standard enthalpies
of formation of the substances in the
reaction. (Example 6.9)
Ch 6 Thermochemistry Review
Pg242-245
Assigned Problems:
# 71, 72, 73, 4, 75, 76
Recommended additional problems:
#33,35!,
Pg246-251
Assigned Problems:
#38, 39, 77, 78, 79, 80, 81, 82, 85, 86,
111, 112, 113,114
Recommended additional problems:
#17,18,19,20,21,83,117!,143!,144!
Ch 6 Thermochemistry Test
Skills List
1 cal = 4.184 Joules
E
k

1
2
mv
2
E  q  w
w  Fd
q  mc t
E  mgh
U
H  H
products
 H
reactants
Hess’s Law
Standard Enthalpies of Formation
Table (pg # )
Kinetic energy
Internal Energy
Law of Conservation of Energy
System
Endothermic Reaction
Enthalpy Change
Specific Heat
Standard Enthalpy of Formation
Potential energy
Joule
Thermodynamics
Surroundings
Enthalpy
Temperature Change
Calorimeter
Energy of Phase Change
How reverse reactions and moles affect
the Enthalpies of formation
New Vocabulary
energy
Chemical Energy
Calorie
Heat of Reaction
Exothermic Reaction
Thermochemical Equation
Molar Heat Capacity
Hess’s Law
Important Dates
11/10
11/11
11/21
11/23
11/24 -11/28
Parent Teacher Conference Day
Veterans Day – No School
Pitt Labs # 1 and 2
Early Dismissal
Thanksgiving Break
UNIT 2: Chapter 6: Thermochemistry
CHS CHEMISTRY
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Chapter 6 Topics and Hints:
Energy, thermochemical equations and stoichiometry, calorimetry, Hess’s law, enthalpy of formation,
Representations:
 Thermochemical equations (balanced equation, followed by ∆H value)
 Energy diagram for reagents and products of a reaction, e.g. Figure 6.8
Dr. Maleckar emphasizes the pure energy portion of the thermos chapter less than what is probably
expected (q and work and energy, etc.) She focuses more on the actual calculation of enthalpy change
relating to reactions and asks questions that are more similar to the ones she has assigned.