Summary
ch.9: thermodynamics (summary notes)
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a summary of the thermodynamics chapter in CHM201.
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TEST BANK FOR CHEMICAL PRINCIPLES 8TH EDITION BY STEVEN S. ZUMDAHL
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Activation Activationdo
( potential kinetic ) the
capacity to •
is
energy or a
•
energy energy
5ro
a a
work or produce heat .
É
e
" EE s
the law of conservation of states that energy
E •
energy
•
*
±
,
g reactant ducts
be
0
can converted from one form to another but can a E- 1-
energy
e " e "
± absorbed
neither be created nor
destroyed g- energy Reactants
- - - - -
§
- -
p-r-o-au.es
-
.
released
☐
MVZ
KE =
d-
°
• *
Reaction Progress Reaction progress
°
as a ball rolls down a hill , some of its kinetic
Exothermic Endothermic
energy is transferred to the surface of the hill as reaction reaction
heat
energy heatingthis transfer of is called frictional DE
°
t w o =q
. .
heat total ) of all mot when
the ( kinetic potential heat absorbed ,
:
energy a - is
ecular motion inside object
an
q=tx
-
.
temperature : is a measure of the
average kinetic
energy -
when heat is released ,
of the particles in an
object g- = ✗
-
.
state function / property refers to
property of the the internal of the
a a DE is
energy system
•
.
depends its state
system that only on present .
surroundings surroundings
is state function , work heat are not
energy a & .
reactants and products of the reaction
system : the
°
reaction container, the Energy Energy
surroundings the room
every
-
: *
,
thing else
-
system system
exothermic : heat flows out of the into
system *
°
AE <0 DE > 0
the
surroundings
endothermic heat flows into a
system Work PAV
°
: =
must When
the
energy lost
by the
system be
equal to is
expanding the system is
°
a
gas
☐
,
the
energy gained by the
surroundings .
doing work on the surroundings . for an ex
-
°
APE is the difference potential energy
in stored in -
panting gas :
the bonds of the products as compared with the -
DV is + ve
bonds of the reactants .
w=
-
P V
the
change in
energy represents the difference when
gas is
being compressed
• °
a :
break bonds in
between the
energy required to the Dv is ve
-
-
reactants and the
energy released when the bonds w is a
positive quantity
the
in the products are formed the
system does work
surroundings
°
. on
in exothermic reaction , the bonds in the when an ideal
gas expands against a constant
•
an
products external
are
stronger than those of the reac pressure
-
.
taints
enthalpy H= Et PV
- •
.
for an endothermic reaction ,
the situation is DH= DE + DPV =
9- p DH = H
products -
H
reactants
reversed .
if the reaction
energy that flows into the system heat DH will be + ve is endothermic
• °
as
is used to 9 the P.E. of the system .
in at constant P * -
ve if the reaction is exo .
this case ,
the products have > P.E. C weaker
bonds on
average ) than the reactants .
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