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Thermodynamics
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Cards (13)
Thermodynamics
The study of the relations between
heat
,
work
,
temperature
, and
energy
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Laws of Thermodynamics
Describe how the
energy
in a
system
change and whether the system can perform
useful
work on its
surroundings
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0th
Law
1. If
two
objects are in
equilibrium
with
another object
, therefore, they are also in equilibrium with each other
2.
Thermal Equilibrium
=
No heat transfer
3. Heat moves from
hot
to
cold
surface
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1st
Law
Law of
Conservation
of Energy.
Energy
can't be
created
nor
destroyed.
It can, however, be
transferred
and
transform
into another form
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2nd
Law
The
entropy
of the universe is always
increasing
Entropy (∆S) is the tendency of a matter to become
disorganized
Everything is doomed for
chaos
and
destruction
Your room will have a chance of becoming
disorganized
as time goes by, but never a chance of it becoming more
organized
on its own
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3rd
Law
The
entropy
of a
crystalline solid
at a temperature of
zero Kelvin
(
absolute zero
) is equal to zero
Solid
has
lesser entropy
than liquid and gas since its particles are more organized
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System
The collection of bodies, matter, or mass that is
being studied
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Surrounding
What's left in the
universe
, except the
system
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Enthalpy
(
∆H
)
The total
internal energy
(
∆U
) of a
system
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Types of Systems
Isovolumetric
:
∆U = Q
, Any change in energy is the result of
heat transfer
,
Constant volume
,
W = 0
Isothermal
:
Q = W
,
Heat
transferred us completely used for
work
,
Constant temperature
,
∆U = 0
Adiabatic
:
∆U = - W
,
Internal energy
is used exclusively for
work
,
No heat transfer
,
Q = 0
Isolated System
:
∆U = 0
, No change in
internal energy
,
Q = 0
,
W = 0
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Gibbs Free Energy
(
∆G)
∆G = ∆H - T∆S
, Tells us about the
spontaneity
of a process
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Gibbs Free Energy Relationships
Spontaneous
: ∆G =
-,
Thermodynamically favorable, Always spontaneous, Never nonspontaneous
Nonspontaneous
: ∆G =
+
, Thermodynamically unfavorable, Always nonspontaneous, Never spontaneous
∆G =
-
, ∆H =
-
, ∆S =
+
,
Energetically favorable
,
Entropically favorable
,
Spontaneous
∆G =
+
, ∆H =
+
, ∆S =
-
,
Energetically unfavorable
,
Entropically unfavorable
,
Nonspontaneous
∆G =
+/-
, ∆H =
+
, ∆S =
+
,
Energetically unfavorable
,
Entropically favorable
, Spontaneous at
high temperature
∆G = +/-, ∆H = -, ∆S = -,
Energetically favorable
,
Entropically unfavorable
, Spontaneous at
low temperature
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Thermodynamic systems can be classified as
open
(exchange
matter
with surroundings),
closed
(
no
exchange of
matter
but exchange
heat/energy
), or
isolated
(
neither
exchanges
matter
nor
energy
).
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