Thermodynamics and Kinetics Guided Notes

67 %
33 %
Information about Thermodynamics and Kinetics Guided Notes
Education

Published on February 15, 2014

Author: emmawise

Source: slideshare.net

Description

Great tool for teaching thermodynamics and kinetics!

Chemistry
Guided
Notes
 
 
 Unit
5:
Thermodynamics
and
Kinetics

 
 
 
 
 
 
 
 
 
 Name:


 Date:

 
 
 
 
 
 
Period:

 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
object
 Energy
  What
is
Energy?
 • Energy‐

 
 
 • Chemical
Potential
Energy‐

  

 
 
 
 
of
atoms
  

 
 
 
 
of
atoms
  

 
 
 
 
of
bonds
 
 
 
 
 
 
 
 
object
to
a

 
  What
is
Heat?
 • Heat
(q)‐

 • Heat
always
flows
from
a

  Warmer
object
losses
energy
in
the
form
of
heat
and
its
temperature


 
 
 
  Cooler
object
gains
energy
in
the
form
of
heat
and
its
temperature

 
 
 
 
 • NOT
THE
SAME
AS
TEMPERATURE
 • Temperature
(T)‐

 • Measuring
Heat:
Two
Units
 
 
 
 
 
 
 
 
 
 
 
  Calorie
(cal)‐

 
 
 
 
 
 
 
 
 
 
 
  Joule
(J)‐

 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 Thermochemistry
and
Enthalpy
  Thermochemistry
 • Thermochemistry‐

 • Universe=
System
+
Surroundings
  System‐

 
 
 
 
 
 
 
 
 
 
 
  Surroundings‐


 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
  Enthalpy
(H)
 • Enthalpy
(H)‐

 
 • Enthalpy
of
a
Reaction
(ΔHrxn)=

 • Thermochemical
equation
are
balanced
equations
that
include
values
for
ΔHrxn
  
 Endothermic
Reactions
 • 
 
 
 
 
 
 
 
 
 
 
 • 

 
 
 
 
 
 
 
 
 
 
 
 •  

 

 
 
 
 
 
 
 
 
 
 
 
 Exothermic
Reactions


• 
 
 
 
 
 
 
 
 
 
 
 
 • 

 
 
 
 
 
 
 
 
 
 
 
 • 

 
 
 
 
 
 
 
 
 
 
 
 
  Hess’s
Law
 • Hess’s
Law‐
states
that
if
you
can
add
two
or
more
thermochemical
reaction
equations
to
produce
a
 final
equation
for
the
reaction
then
the
sum
of
the
enthalpy
changes
for
the
individual
reactions
is
 the
enthalpy
change
for
the
final
reaction
 
 • Three
Rules:

  If
the
reaction
must
be
doubled,

 
 
 
 
 
 
 
 
  If
the
reaction
must
be
reversed,

 
 
 
 
 
 
 
 
  Anything
on
both
sides
of
the
final
equation
can
be

 
 
 
 
 
 
 
 • Example:
Calculate
the
ΔH
for
the
reaction
2S
(s)
+
3
O2
→
2SO3
(g)
using
the
information
below.
 a. 2SO3
(g)
→
2SO2
(g)

+
O2
(g)

 
 ΔH=
198
kJ
 b. S
(s)
+

O2
→
SO2
(g)
 
 ΔH=
‐297kJ
 
 
  SO3
is
on
the
product
side
of
the
desired
equation
so
reverse
reaction
a.
 
 
 
  The
coefficient
of
the
1st
reactant,
S
(s)
is
2
in
the
desired
equation.
Therefore,
reaction
b
 must
be
doubled.
 
 
 
  Add
the
equations
together
and
cancel
anything
that
occurs
on
both
the
reactant
and
 product
side.
 
 
 
  Write
the
final
equation
for
the
reaction
including
the
ΔH
value.
Box
or
Circle.
 
 
 
 Spontaneity,
Entropy,
Enthalpy,
and
Gibb’s
Free
Energy


 Spontaneity
 • Spontaneous
Processes‐

 
 
 
 
 
 
 
 
 
 
 • Nonspontaneous
Processes‐

 
 
 
 
 
 
 
 
 
 
  Entropy
(S)
 • Entropy
(S)‐
 
 
 
 
 
 
 
 
 
 
 
 
 • 2nd
Law
of
thermodynamics‐

 
 
 
 
 
 
 
 
 
 

 
 
 
 
 
 
 
  Gibb’s
Free
Energy
(G)
 • Gibb’s
Free
Energy
(G)‐

 
 
 
 • Relates

 
 
 
and
can
be
used
to
predict
reaction
spontaneity

 • Formula
for
Gibb’s
Free
Energy:
 
 
and

 
 
 
 
  
 
 
 
 
 
 
 
 
  • If
ΔG
value
is
negative,


 If
ΔG
value
is
positive,


 
 
 
 
 
 
 
 
 
 Spontaneity,
Enthalpy,
and
Entropy
 
 Exothermic
Reaction
(­ΔH)
 Endothermic
Reaction
(+ΔH)
 
 
 
 Increased
Entropy
(+ΔS)
 
 
 Decreased
Entropy
(­ΔS)
 
 
 
 Specific
Heat
  Specific
Heat
(c)
 • Specific
Heat
(c)‐


 
 
 
 
 
 
 
 
 
 
 
 • 

 
 
 
 
 
 
 
 
 
 
 
 • Substances
with
high
specific
heat
 
 
  
 
 
 
 
 
 
 
 
 
 
 
  

 
 
 
 
 
 
 
 
 
 
 
 
  • 


 

 
 
 
 
 
 
 
 
 
 
 
 
 Substances
with
low
specific
heat
  


 
 
 
 
 
 
 
 
 
 
 
 
  

 
 
 
 
 
 
 
 
 
 
 
 
  

 
 
 
 
 
 
 
 
 
 
 
 
 


• Formula
for
Calculating
Heat
Released
or
Absorbed:
 
 
 • if
the
value
for
q
is
negative,

 
 
 
 
 
 
 
 
 •  q‐

 
 
 
 
 if
the
value
for
q
is
positive,

 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
  m‐

 
 
 
 
 
 
  c‐
 
 
 
 
 
 
  ΔT‐

 
 
 
 
 
 
 
 
 
 
 
must
be
absorbed
by
the

  Law
of
Conservation
of
Energy
 • Law
of
Conservation
of
Energy‐

 • 1st
Law
of
Thermodynamics
 • Heat
lost
by
the


 
 
 
 
 
 • Heat
transfer
is
measured
using
a
device
called
a
calorimeter
 
 
 
 
 
 
 
  Specific
Heat
Example
Problems
 • • Example
1:
Calculating
Heat‐
If
the
temperature
of
34.4g
of
ethanol
increases
from
25.0°C
to
78.8°C,
 how
much
heat
has
been
absorbed
by
the
ethanol?
(The
specific
heat
of
ethanol
is
2.44J/g°C)
 
 
 
 
 
 
 
 
 Example
2:
Calculating
Temperature‐
A
4.50g
nugget
of
pure
gold
absorbed
267J
of
heat.
What
was
 the
final
temperature
of
the
gold
if
the
initial
temperature
was
25°C?
(The
specific
heat
of
gold
is
 0.129J/g°C.)
 
 
 
 
 
 


• Example
3:
Calculating
Specific
Heat‐
A
155g
sample
of
an
unknown
substance
was
heated
from
 25.0°C
to
40.0°C.
In
the
process,
the
substance
absorbed
5696
J
of
energy.
What
is
the
specific
heat
 of
the
substance?

 
 
 
 
 
 
 
 
 Activation
Energy
and
Reaction
Rates
 
  Reaction
Energy
Diagrams
 Reaction Progress Reaction Progress  Activation
Energy
 Activation
Energy
(EA)‐

 
 
 
 
 
 
 
 
 
 
 • 
 
 
 
 
 
 
 
 
 
 
 
 
 • Reaching
the
activated
complex
requires

 
 
 
 
 
 
 
 
 • High
activation
energy
correlates
to
a


 
 
 
 
 
 
 
 
 • Low
activation
energy
correlates
to
a

 
 
 
 
 
 
 
 
 
  Factors
that
Affect
Reaction
Rates
 • Nature
of
Reactants‐

 
 
 
 
 
 
 
 
 
 
 
 • Concentration‐

 
 
 
 
 
 
 
 
 
 
 
 • Surface
Area‐

 
 
 
 
 
 
 
 
 
 
 
 
 • Temperature‐

 
 
 
 
 
 
 
 
 
 
 
 Catalyst‐

 
 
 
 
 
 
 
 
 
 
 
 • 
 
 
 
 


Add a comment

Related presentations

Related pages

GUIDED NOTES, a.k.a. How much stuff is in this unit!?!?

GUIDED NOTES, a.k.a. ... Unit 9: Fluid Mechanics and Thermodynamics ... C. Kinetic theory and thermodynamics 1. Ideal gases a.
Read more

Honors Chemistry - Mrs. lallemand’s web site

Honors Chemistry Syllabus: H Chemistry Syllabus.docx. ... Unit 5 Guided Notes: Thermodynamics and Kinetics Guided Notes.pdf. Unit 5 PowerPoint: ...
Read more

Unit 5: Thermodynamics and Kinetics Name: Table of ...

Unit 5: Thermodynamics and Kinetics Guided Notes N/A 5 Hess’s Law ... Thermodynamics and Kinetics Study Guide H 18 Title ...
Read more

GUIDED NOTES - Mrs. B's Physics Fabulousness

GUIDED NOTES Unit 9: Thermodynamics OBJECTIVES ... During average collisions between molecules, kinetic energy is transferred from faster molecules
Read more

Chem 3070: Thermodynamics and Kinetics. Spring 2013

Chem 3070: Thermodynamics and Kinetics. ... A Guided Inquiry: Thermodynamics & Statistical ... (Note that this is not the same order in which they are ...
Read more

Notes, Chapter 17: Equilibrium & Kinetics

Equilibrium & Kinetics Notes, Chapter 17 . ... thermodynamics, kinetics, and equilibrium. Thermodynamics was covered in Pt. I. I. Kinetics.
Read more

Name Period AP Biology Date RAVEN CHAPTER 8 GUIDED NOTES ...

RAVEN CHAPTER 8 GUIDED NOTES: ... a. kinetic energy ... Explain the First Law of Thermodynamics and its relationship to biological ...
Read more

Chem 406: Lecture Notes - University of Wisconsin–Eau Claire

Reading Assignment: Hammes, G; Thermodynamics and Kinetics for the Biological Sciences; Chapter 2 - Entropy and Free Energy ... Lecture Notes ...
Read more

Problems In Metallurgical Thermodynamics And Kinetics Pdf

METALLURGICAL THERMODYNAMICS AND KINETICS ... 618 reads chapter 17 section 2 the war for europe north africa notes ... 668 reads american history guided ...
Read more