Thomas Jefferson

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Thomas Jefferson

• On his tombstone
• Jefferson asked that only three of his many
  accomplishments be engraved on his tombstone
  Author of the Declaration of American
  Independence Author of the Virginia Statute for
  Religious Freedom and Father of the University
  of Virginia

Born April 13, 1743 Died July 4, 1826
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Attended (1760-62) the College of William and
Mary and then studied law
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He was a quiet man however he wrote with
incredible power

• Known as the silent member of congress

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His writings and quotes are incredible

• Determine never to be idle...It is wonderful how
  much may be done if we are always doing.
• Thomas Jefferson

Nothing gives one person so much advantage over
another as to remain always cool and unruffled
under all circumstances. Thomas Jefferson
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Learn to write and be careful what you read
Advertisements contain the only truths to be
relied on in a newspaper. Thomas Jefferson

• I do not take a single newspaper, nor read one a
  month, and I feel myself infinitely the happier
  for it.
• Thomas Jefferson

I'm a great believer in luck, and I find the
harder I work the more I have of it. Thomas
Jefferson
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Water was always a problem at Monticello. After
all, Monticello is on top of a mountain. Wells
were dug but they proved unreliable. Jefferson
collected run-off rainwater from the terraces off
the back of Monticello. He installed gutters on
the terraces and directed the collected water
into cisterns.
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Architect statesmen and philanthropist
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HomeworkRead 423 to 435Do problems 1 -12 on
page 4321-4 page 435
Gas law handout Lecture 38
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We've studied Basic Bonds

• Ionic clean plus and minus
• Covalent sharing of electrons
• a) dipoles
• b) hydrogen
• c) London
• Metallic sea of electrons (delocalized)

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The tighter the bondsthe higher the melting or
boiling point

• Ionic and metallic tight
• Covalent lower electronegativity
  difference of 2.1 or below
• London weakest bond

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Note Web quiz practice lec 37
What kind of bond ionic, dipole dipole,
London, hydrogen bond

• CH3OH
• H2O CH3CH2CH2CH3
• CH4
• NH3 CH3OCH3
• I2
• Fe
• CO2
• NaCl

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Most recently we have studied gases where the
degree of vaporization is dependent on 1)
ambient pressure2) vapor pressure

• Greater ambient pressure greater vapor pressure
  necessary for boiling

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We also saw how the kinetic molecular theory
explains the properties of gases and how Dalton
showed how vapor pressures are additive
Ptotal P1 P2 P3
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And last time we spoke of how we use Charless
law where you have to use Temperature in Kelvin
to establish the simple temperature to volume
ratio
Celsius 273 Kelvin
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http//dbhs.wvusd.k12.ca.us/GasLaw/WS-Charles.html

• A gas occupies 900.0 mL at a temperature of 27.0
  C. What is the volume at 132.0 C?
• What change in volume results if 60.0 mL of gas
  is cooled from 33.0 C to 5.00 C?
• 3) Given 300.0 mL of a gas at 17.0 C. What is
  its volume at 10.0 C?

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What if you decrease the volume of a gas what
happens to the temperature

• We know that if you decrease the temperature the
  volume decreases

Direct relationship
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So Charles studied volume and temperature

• What about pressure and volume

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Boyles Law

• Boyle did experiments on the relationship
  between pressure and volume

If you double the volume of a container that
holds a gas what will happen to the pressure
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Bell Jar and balloon
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(No Transcript)
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Boyle found that there was a direct relationship
between volume and pressure

• P1V1 P2V2

Dont memorize this equation
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Show Corsican diver

• Relate to water pressure

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We talked about Dalton's law of partial pressure
We also discussed Charles law that stated that
as the temp changes the volume changes
We also discussed Boyles law that stated that as
you increase pressure you decrease volume
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We discussed how an increase in the number of
atoms (n) the more pressure
?n ?P
But do all particles yield the same
pressure!!!!!!!

• NO

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• These guys dont push with the same pressure

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• C(?n) ?P

Where n is the number of atoms and C is a
constant depending how big the atoms are.
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So we have all these different laws

• P1V1P2V2

V1/T1 V2/T2
P (C) n
Putting them all together you get
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Ideal gas law

• Accumulation of all the gas laws into one law

This you memorize
PV nRT
P pressure atm V volume
liters N number of moles T temperature in
Kelvin R is the universal gas constant .0821 L.
Atm /mole K.
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Ideal gas law
Remember to check your units against the
universal gas constant units

• Accumulation of all the gas laws into one law

This you memorize
PV nRT
P pressure atm V volume
liters N number of moles T temperature in
Kelvin R is the universal gas constant .0821. Atm
L /mole K.
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Dont Memorize R you will be given this on all
exams

• But check the units
• R 6.24 x 104 L mmHg/mol K

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When doing the problems remember to

• a)     rearrange the ideal gas law to solve for
  variable
• b)    change known issues to proper labels moles
  atm liters K
• c)     do math

PvnRT
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Calculate the pressure of 1.0 g of hydrogen gas
at 160C and occupy a volume of 2.54 L

•  
• Rearranging the ideal gas law to solve for P you
  get PnRT/V

Change the values to moles kelvin liters R
.0821atm(L)/molesK
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II How many moles of nitrogen gas are there in
0.38 liter of gas at 0OC and 380 mm Hg pressure

• T C 273
•  
• P 760Torr 1 atm

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III What is the pressure in atmospheres exerted
by a .500 mole sample of nitrogen gas in a 10 L
container at 298K ?
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Example IV What pressure, in atm is exerted by
0.325 mole of hydrogen gas in a 4.08 L container
at 35 C
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Example V What mass of chlorine gas Cl2 in
grams. is contained in a 10 liter Tank at 27oC
and 3.50 atm of pressure? 
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Example VI What is the volume of 71 grams of
chlorine gas Cl2 at 0 oC and 1 atm of
pressure? 

• Example VII What is the volume of 2 grams of
  Hydrogen gas H2 at 0 oC and 1 atm of pressure?

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Do the ideal gas Law handout
Honors finish this for homework
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