Chapter 5 Thermochemistry - Yolaclassfiles.yolasite.com/resources/Week 1_Part 1...27/12/2011 1...
Transcript of Chapter 5 Thermochemistry - Yolaclassfiles.yolasite.com/resources/Week 1_Part 1...27/12/2011 1...
27/12/2011
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Chapter 5
Week 1
Part 1
Thermochemistry
John D. Bookstaver
St. Charles Community College
Cottleville, MO © 2012 Pearson Education, Inc.
Thermochemistry
© 2012 Pearson Education, Inc.
Energy
• Energy is the ability to do _________ or __________ _______.
– Energy used to cause an object that has mass to _______ is called ____________. (W = ____ x ___)
– Energy used to cause the _____________ of an object to _____ is called _________.
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Thermochemistry
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Kinetic Energy
Kinetic energy is energy an object
possesses by virtue of its ___________:
Ek = ________
Thermochemistry
Potential Energy
• Potential energy is energy __________,
for example in a _________ or
________ ________.
E = ________
• Where m = mass, h = height and g =
gravity constant
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Thermochemistry
© 2012 Pearson Education, Inc.
Potential Energy • Potential energy is
energy an object possesses by virtue of its _________ or chemical composition. It is stored energy that arises from ________ and repulsions an object experiences in relation to another object.
• The most important form of potential energy in molecules is __________ potential energy, Eel:
Eel = ___________
Thermochemistry
© 2012 Pearson Education, Inc.
Units of Energy
• The SI unit of energy is the ______ (_):
• An older, non-SI unit is still in
widespread use: the _______ (___):
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Thermochemistry
What is a BTU?
• BTU (______ ______ ____) – it is
based on the _______ of heat required
to rise the temperature of __ pound of
water to __̊ F.
1 BTU = ____________Joules
You must ___________ these energy
conversions! © 2012 Pearson Education, Inc.
Thermochemistry
Convert the following:
1. ___ BTU to Joules
2. _____ BTU to kcal
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Thermochemistry
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First Law of Thermodynamics
• Energy is neither _________ nor _________.
• It can only be _______________ from one form
to another.
Thermochemistry
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Conversion of Energy Figure 5.2
• Energy can be converted from one type to
another.
• For example, the cyclist has _______ energy
as she sits on ____ of the _____.
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Thermochemistry
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Conversion of Energy
• As she coasts ______ the hill, her potential
energy is converted to __________ energy.
• At the bottom, all the potential energy she
had at the top of the hill is now kinetic energy.
Thermochemistry
Conversion of Energy
• Consider a car in motion
_______ energy
• You suddenly apply the ________, what
happens to the energy?
Kinetic energy is converted to ______
energy (_______ pads heat up, ________
from the road produces ______)
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Thermochemistry
First Law of Thermodynamics
• To understand the movement of energy
we must first define the _______ and its
_________________.
• In the laboratory the _________ is the
________ and _______ of the chemical
mixture (the system is the reaction what
you are investigating)
• The ____________ is the container and
everything beyond
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Thermochemistry
© 2012 Pearson Education, Inc.
Example: System and Surroundings
• The system includes the
molecules we want to
study (here, the hydrogen
and oxygen molecules).
• The surroundings are
_________ _____ (here,
the cylinder and piston).
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Thermochemistry
Types of Systems
1. ______ – matter and energy can be
__________ with the ______________
2. ______ – can exchange energy but
_____ matter with the _____________
3. ______ – _______ energy or matter
can be exchanged with the _________
© 2012 Pearson Education, Inc.
Thermochemistry
© 2012 Pearson Education, Inc.
First Law of Thermodynamics
• Energy is neither created nor destroyed.
• In other words, the total energy of the _______ is
a constant; if the system _____ energy, it must
be _______ by the surroundings, and vice versa.
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Thermochemistry
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Exchange of Heat between System and
Surroundings
• When heat is ________ by the ________ from
the surroundings, the process is ___________.
• When heat is ________ by the _________ into
the surroundings, the process is ___________.
Thermochemistry
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Internal Energy
• The _________ ________ of a system is the
sum of all ________ and ________ energies of
all components of the system; we call it E.
• The internal energy of a substance can be due to
________________, ____________ (kinetic
energy) and ____________ \ _________ forces.
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Thermochemistry
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Internal Energy
By definition, the change in internal energy, E,
is the final energy of the system minus the initial
energy of the system:
E = ______ − ______
Thermochemistry
© 2012 Pearson Education, Inc.
Changes in Internal Energy
• If _____ > ___, _____ > ______
– Therefore, the system __________ energy from the surroundings.
– This energy change is called __________.
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Thermochemistry
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Changes in Internal Energy
• If ____ < __, _____ < _____
– Therefore, the system ________ energy to
the surroundings.
– This energy change is called __________.
Thermochemistry
© 2012 Pearson Education, Inc.
Changes in Internal Energy
• When energy is
exchanged between
the _______ and the
____________, it is
exchanged as either
heat (__) or work
(___).
• That is,
E = __ + __.
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Thermochemistry
Internal Energy – Sign of “q”
• Sign reflects the system’s point of view is
energy flowing into or out of the system?
• ___________ Process – energy flows _____
the system:
q is ___________
• ___________ Process – energy flows _____
of the system:
q is ___________
Thermochemistry
Internal Energy – Sign of “w”
• Sign reflects the system’s point of view.
• System _____ _____ on ______________
example, blowing up a balloon, it
_______ into the surrounding:
w is ________ energy flows ____ of
system
• Surroundings do work on the system:
w is ________ energy flows _____
system
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Thermochemistry
© 2012 Pearson Education, Inc.
Let’s Consider “Work”
Usually in an open
container the only work
done is by a gas
pushing on the
surroundings (or by
the surroundings
pushing on the gas).
Thermochemistry
© 2012 Pearson Education, Inc.
Determing the Sign for “Work” We can measure the work done by the gas if
the reaction is done in a vessel that has been
fitted with a piston:
w = _____ and ∆V = _______ - _______
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Thermochemistry
© 2012 Pearson Education, Inc.
E, q, w, and Their Signs
Thermochemistry
Example 1:
• Calculate the change in the internal
energy for a process in which a system
absorbs ____ J of heat from the
surroundings and does ____ J of work
on the surroundings.
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Thermochemistry
Example 2:
• One gram of liquid water absorbs ____J
of heat and is converted to steam. The
steam ______ and does _____J of work
on a turbine blade. Calculate q, w and
∆E.
© 2012 Pearson Education, Inc.
Thermochemistry
Example 3:
• A balloon is heated by adding _____J of
heat. It ______, doing ____J of work on
the atmosphere. Calculate ∆E.
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Thermochemistry
First Law of Thermodynamics
• 5.13, 5.15, 5.19, 5.25, 5.27
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Thermochemistry
References:
• Brown, T.L., Bursten, B.E., LeMay, H.E., Murphy, C.J.
and Woodward, P.M. (2012). Chemistry – The Central
Science. (12th ed.). United States Of America: Pearson
Prentice Hall
• Brown, T.L., Bursten, B.E., LeMay, H.E. and Murphy,
C.J. (2009). Chemistry – The Central Science. (11th
ed.). Upper Saddle River, NJ: Pearson Prentice Hall.
• Zumdahl, S.S. and Decoste, D.J. (2010). Introductory
Chemistry: A Foundation. (7th ed.). Belmont, CA:
Brooks/Cole Cengage Learning.