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Lecture 1: Energy and Enthalpy
• Reading: Zumdahl 9.1 and 9.2
• Outline– Energy: Kinetic and Potential– System vs. Surroundings– Heat, Work, and Energy– Enthalpy
• Energy is the capacity to do work or to produce heat
• Energy is conserved, it can neither be created nor destroyed, different forms of energy interconvert
• However, the capacity to utilize energy to do work is limited (entropy)
Energy: Kinetic vs. Potential
• Potential Energy (PE)– Energy due to position or
chemical composition
– Equals (mgh) in example.
• Kinetic Energy (KE)– Energy due to motion.
– Equals mv2/2 in example.
h
m
v
Mechanical Energy = KE + PE
• Energy is the sum of kinetic energy and potential energy.
• Energy is readily interconverted between these two forms.
• If the system of interest is isolated (no exchange with surroundings), then total energy is constant.
Example: Mass on a Spring• Initial PE = 1/2 kx2
• At x = 0:– PE = 0– KE = 1/2mv2=1/2kx2
• Units of EnergyJoule = kg.m2/s2
• Example:– Init. PE = 10 J– M = 10 kg– Vmax = [2(PE)/M]1/2 = 1.4m/s
0
Energy: Kinetic vs. Potential
• Potential Energy (PE)– Energy due to position or
chemical composition
– Equals (mgh) in example.
• Kinetic Energy (KE)– Energy due to motion.
– Equals mv2/2 in example.
h
m
v
First Law of Thermodynamics
First Law: Energy of the Universe is Constant
E = q + w
q = heat. Transferred between two bodies of differing temperature. Note: q ≠ Temp!
w = work. Force acting over a distance (F x d)
Applying the First Law
• Need to differentiate between the system and surroundings.
• System: That part of the universe you are interested in (i.e., you define it).
• Surroundings: The rest of the universe.
System
Surroundings
q transfer
w transfer
Conservation of Energy
• Total energy is conserved.
• Energy gained by the system must be lost by the surroundings.
• Energy exchange can be in the form of q, w, or both.
P = 1atm
P = 1atm
Initial
Final
Heat Exchange: Exothermic
• Exothermic Reaction. Chemical process in which system evolves resulting in heat transfer to the surroundings
• Heat flows out of the system
• q < 0 (heat is lost)
Ene
rgy
Ene
rgy Einitial
Efinal
Efinal < Einitial
Water @ 80° C
Water @ 20° C
q
Heat Exchange: Endothermic
• Endothermic Reaction: Chemical process in which system evolves resulting in heat transfer to the system
• Heat flows to the system
• q > 0 (heat is gained)
Ene
rgy
Ene
rgy
Einitial
Efinal
Efinal > Einitial
Water @ 80° C
Water @ 20° C
q
• In exothermic reactions, the potential energy stored in chemical bonds is converted into thermal energy (random kinetic energy), i.e. heat
• Once we have done that, we have lost the ability to utilize the same potential energy to do work or generate heat again (dissipation)
Energy and Sign Convention
• If system loses energy:
Efinal < Einitial
Efinal-Einitial = E < 0.
• If system gains energy:
Efinal > Einitial
Efinal-Einitial = E > 0.
Ene
rgy
Ene
rgy
Ene
rgy
Einitial
Efinal
E > 0
Ein
Ene
rgy Einitial
Efinal
E < 0
Eout
Heat and Work Sign Convention
• If system gives heat
q < 0 (q is negative)
• If system gets heat
q > 0 (q is positive)
•If system does work
w < 0 (w is negative)
•If work done on system
w > 0 (w is positive)
Example: Piston
• Figure 9.4, expansion against a constant external pressure
• No heat exchange: q = 0• System does work: w < 0
(adiabatic)
Example (cont.)• How much work does the
system do?
• Pext = force/area
• |w| = force x distance
= Pext x A x h
= Pext V
• w = - Pext V (note sign)
• When it is compressed, work is done to a gas
• When it is expanded, work is done by the gas (e.g. your car’s engine)
Example 9.1
• A balloon is inflated from 4 x 106 l to 4.5 x 106 l by the addition of 1.3 x 108 J of heat. If the balloon expands against an external pressure of 1 atm, what is E for this process?
• Ans: First, define the system: the balloon.
Example 9.1 (cont.)
E = q + w
= (1.3 x 108 J) + (-PV)
= (1.3 x 108 J) + (-1 atm (VfinalVinit))
= (1.3 x 108 J) + (-0.5 x 106 l.atm)
• Conversion: 101.3 J per l x atm
(-0.5 x 106 l.atm) x (101.3 J/l.atm) = -5.1 x 107 J
Example 9.1 (cont.)
E = (1.3 x 108 J) + (-5.1 x 107 J)
= 8 x 107 J (Ans.)
The system gained more energy through heat than it lost doing work. Therefore, the overall energy of the system has increased.
Definition of Enthalpy
• Thermodynamic Definition of Enthalpy (H):
H = E + PV
E = energy of the system
P = pressure of the system
V = volume of the system
Why we need Enthalpy?
• Consider a process carried out at constant pressure.
• If work is of the form PV), then:
E = qp + w
= qp - PV
E + PV = qp
qp is heat transferred at constant pressure.
Definition of Enthalpy (cont.)
• Recall: H = E + PV
H = E + PV) = E + PV (P is constant)
= qp
• Or H = qp
• The change in enthalpy is equal to the heat transferred at constant pressure.
Changes in Enthalpy• Consider the following expression for a chemical process:
H = Hproducts - Hreactants
If H >0, then qp >0. The reaction is endothermic
If H <0, then qp <0. The reaction is exothermic