may 7, 2012 honors chemistry brain teaser turn in titration lab describe the characteristics or...
TRANSCRIPT
Brain Teaser
Turn in Titration Lab Describe the characteristics or
properties of solid, liquid and gases
Agenda
Brain Teaser Unit 9 Acid/Base Test Result Notes: Introduction to Gases and Gas Laws Homework
Charles and Boyles Law Worksheet
Introduction to GasesIntroduction to Gases
Earth is surrounded by a layer of gaseous molecules - the atmosphere - extending out to about 50 km.
Characteristics of GasesCharacteristics of Gases
Gases low density; compressible volume = shape of container expand when heated large distance between particles
Model of a gas: rapidly moving particles: vol. & shape of container no attraction between particles moving about freely large space between particles: low density & high
compressibility
12m05vd112m05vd1
12m05vd1.mov.lnk
gas_particle_motion.exe.lnk
Liquids and SolidsLiquids and Solids
Liquids higher density, lower compressibility characteristic volume; shape of container particles closer together; moving about;
experience attractive forces Solids
high density; low compressibility particles are close together; little empty
space; strong attractive forces characteristic volume and shape
Atomic View of the States of MatterAtomic View of the States of Matter
Note distance between particles and order of arrangement of particles
Figure 9.101m07an101m07an1
01m07an1.mov.lnk
atomdemo.exe.pif
A10-1-19.mov.lnk
PressurePressure
Pressure = force/area Units: lb/ft2
Pa = N/m2 = kg/ms2
torr = mm Hgatm
1 atm = 760 torr= 760 mm Hg1 atm = 29.9 in Hg = 14.7 lb/in2
1 atm = 101.3 kPa Measure pressure with barometer or U-
tube or manometer
gas_pressure.exe.lnk
Charles’ Law- Relationship between:_________ and __________
Variables/Units
Held Constant
Relationship (direct or inverse)
In words
T = K V = L P = atm n = moles
Direct
As temperature increases, volume increases
Charles’ Law
Charles’ Law Formula
How to convert
C to K
F to C to K
V/T = m m= constant V1/T1 = V2/T2
K = C + 273
C = 5/9(F-32) K = C + 273
Charles’ Law
Temperature
Conversion Practice
Practice Problem
Convert 212 degrees F to K
Convert 50 degrees C to K
The volume of a sample of gas is 2.50L at 45K. What is the volume when it is heated to 125K at a constant pressure.
Boyle’s Law: The relationship between _______ & ________
Variables/Units
Held Constant
Volume (L) Pressure (atm)
Temperature (K) Moles (n)
Boyle’s Law:
Relationship (direct or inverse)
Relationship in words
Inverse
As pressure increases volume decreases.
Boyle’s Law Formula
Boyle’s Law Formula
Pressure Units
PV = m m = constant P1V1 = P2V2
atm = atmospheres mmHg = millimeters of mercury torr Pa = Pascals psi = pounds per square inch 1 atm = 101,325Pa = 760 mmHg
= 760 torr = 14.70psi
Boyle’s Law
How to convert from pressure units to atm
(use dimensional analysis)
Convert 458mmHg to atm
Convert 96.5 psi to atm
Convert 485kPa to atm
Boyle’s Law
Boyle’s Law Practice Problem
The pressure on 2.5L of anesthetic gas is changed from 760mmHg to 304mmHg. What will be the new volume of the gas?
Open Note Quiz (5/6) Place Homework on your desk
Textbook Notes Charles and Boyles’ Laws Worksheet
Time – 10 minutes
Unit Conversion for Gas Laws Calculations
Convert to the following unitsP = atm
V = Liters
T = Kelvin (oC + 273)
Brain Teaser
The pressure on 5.5 L gas is changed from 3 atm to 5 atm. What will be the new volume of the gas?
The volume of a sample of gas is 4 mL at 40oC. What is the volume when it is heated to 60 oC at a constant pressure?
Agenda
Brain Teaser Grade Worksheet: Charles and Boyles’
Law Worksheet Notes: Combined Gas law, Avogadro’s
Law and Ideal Gas Law Homework
Ideal Gas Law and Combined Gas Law Worksheet
2
2
1
1
0
)(
n
V
n
V
mn
V
b
bnmV
Avogadro’s Law If the pressure and temperature are held
constant, the volume of a gas is directly proportional to the number of moles (n).
V
n
Gas Laws Part 2: Work on Gas Notes Sheet instead of Brain Teaser
Avogadro’s Law
O2 O3
Suppose we have a 12.2 L sample containing 0.50 mol oxygen gas at a pressure of 1 atm and a temperature of 25 ºC.
1) Balance the equation2) If all this oxygen is converted to ozone at the same
temperature and pressure, what would be the volume
of the ozone?
Dalton’s Law Practice
A mixture of oxygen, carbon dioxide, and nitrogen has a total pressure of 0.97atm. What is the partial pressure of Oxygen, if the partial pressure of carbon dioxide is 0.70atm and the partial pressure of nitrogen is 0.12atm?
The Gas LawsThe Gas Laws
Variables: V, P, T, n (or m and MM or d)
Ideal Gas: properties are independent of the identity of the gas
What is the relationship between the variables for an ideal gas?
Basketball Bike Tire
5.3 Ideal Gas Law
PV = nRT P= pressure V = volume n = number of moles R = ideal gas constant
0.08206 L·atm/mol·K T = temperature
STP
Standard Temperature and Pressure 0ºC and 1 atm
Use the Ideal Gas Law to calculate the volume of 1.00 mol of gas at STP
Molar Volume at STP
We can show that 22.414 L of any gas at 0C and 1 atm contain 6.02 1023 gas molecules.
Example
A sample of Hydrogen gas has a volume of 8.56 L at 0ºC and a pressure of 1.5 atm. Calculate the moles H2 molecules present in this gas sample.
Practice ProblemPractice Problem
The volume of an oxygen cylinder is 1.85 L. What mass of oxygen gas remains in the cylinder when it is “empty” if the pressure is 755 torr and the temperature is 18.1oC?
Answer: 2.46 g
Gas Law Stoichiometry
Quicklime (CaO) is produced by the thermal decomposition of calcium carbonate. Calculate the volume of CO2 at STP produced from the decomposition of 152 g of CaCO3 by the reaction
CaCO3 (s) CaO (s) + CO2 (g)
Molar Mass and the Ideal Gas Law
If 0.126 g of a gas are contained in a 25mL tank at 25ºC and 3.25 atm, what is the molar mass of the gas? What is the gas?
Kinetic Molecular Theory A model that attempts to explain the behavior of an
ideal gas. The particles are so small that compared with the
distances between them that the volume of the individual particles can be assumed to be negligible (zero).
The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas.
Kinetic Molecular Theory
The particles are assumed to exert no forces on each other; they are assumed to neither attract nor repel each other.
The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.
When does the Kinetic Molecular Theory break down?
What conditions would cause our assumptions to become in valid?
Derivations from the Ideal gas law:
Derivations occur in non-ideal conditions such as low temperature or high pressure:
At high density the volume of the particles themselves become important.
Gas particles do attract each other when they are close together.
BarometerBarometer
What is in a vacuum? What is the weight of the atmosphere?
Figure 9.3
atmospheric_pressure.exe.lnk
Charles’ Law As x increases, y stays
the same, no relationship. y = b y is constant
As x increases, y increases
Y = mx + b
As x increases, y decreases
Y = m(1/x) + b
Team
A sample of nitrogen occupies a volume of 250 mL at 25ºC. What volume will it occupy at 95ºC.
Fluorine gas at 300 K occupies a volume of 500 mL. To what temperature should it be lowered to bring the volume to 300 mL?
Pop Quiz: Boyle’s Law
Sulfur dioxide, a gas that plays a central role in the formation of acid rain, is found in the exhaust of automobiles and power plants. Consider a 1.53 L sample of gaseous sulfur dioxide at a pressure of 5.6 x 103 Pa. If the pressure changed to 0.148 atm at a constant temperature, what will be the new volume of gas?