Transcript Gases - Mounds View School Websites
Gases
Chapter 14
Properties of Gases as demonstrated by experiments • Gases have mass • Gases exert pressure • Gases can expand to take up large volumes • Gases can be compressed to fit in small volumes
• • • •
Kinetic Molecular Theory
The gas consists of very small particles, all with non-zero mass . These molecules are in constant, random motion . The rapidly moving particles constantly collide with the walls of the container. The collisions of gas particles with the walls of the container holding them are perfectly elastic. The interactions among molecules are negligible . They exert no forces on one another except during collisions.
Boyle’s Law
• Boyle’s law states that
at constant temperature
, the absolute pressure and the volume of a gas are inversely proportional. Meaning, as pressure increases, volume decreases.
• For Example: http://www.grc.nasa.gov/WWW/K12/airplane/aboyle.html
Symbolic Representation of Boyle’s Law
Pressure (kPa) • As pressure increases, volume decreases.
Volume (L) • P * V = constant • So, P 1 V 1 = P 2 V 2
Measuring pressure
• Many ways to measure pressure of a gas.
– Atmospheres (atm) force per unit area exerted against a surface by the weight of air above that surface in the Earth’s atmosphere.
– mm Hg (mmHg) pressure of 1 mm of mercury in a column of mercury.
– torr equal to 1 mmHg – pascals or kilopascals
Measuring pressure in Chemistry class
• Pascals (Pa) or kilopascals (kPa) • 1 Pa = the amount of force 1 kg exerts on 1 m 2 for every 1 s 2 .
1 Pa = 1 x 10 -6 atm
• 1 kPa = the amount of force 1000 kg exerts on 1 m 2 for every 1 s 2 .
1 kPa = 1 x 10 -3 atm
Boyle’s Law Problem
• A balloon contains 20.0 L of helium gas at 103kPa. The balloon rises to an altitude where the pressure is only 15.0 kPa. What happens to the volume of the balloon?
P 1 V 1 = P 2 V 2 P 1 = 103 kPa V P 2 1 = 20.0 L = 15.0 kPa V 2 = ?
(103kPa)(20.0L) = (15.0kPA)V2
Charles’ Law
• When pressure is held constant, the volume and temperature of a gas are directly proportional. Meaning as temperature increases, volume increases.
• For example, http://www.wisc-online.com/objects/index_tj.asp?objID=GCH1704 • http://www.youtube.com/watch?v=ZvrJgGhnmJo
Symbolic Representation of Charles’ Law
Volume (L) • As temperature increases, volume increases.
Temperature (K) • So, V/T = constant
V
1
T
1
V
2
T
2
Measuring Temperature
• • •
Fahrenheit
– (based on the freezing and melting point of water)
Celsius
– (based on the freezing and melting point of water but in base 10)
Kelvin
– (based on the idea that at 0 Kelvin or absolute zero, atoms are
NOT
in motion)
Converting between Celsius and Kelvin
• Kelvin, K = o C + 273 So, 32 o C = 32 + 273 = 305 K • 100 o C = 100 + 273 = 373 K
Charles’ Law Practice
• A balloon has a volume of 1.00 L. The temperature of the room where the balloon is located is 273 K. If the room is heated to 300 K, what happens to the volume of the balloon?
Make a
qualitative
assessment of what is going to happen to the volume of the balloon after an increase in temperature.
V
1
T
1
V
2
T
2 1 .
00
L
273
K
V
2 300
K
Gay Lussac’s Law
• If the volume is constant, as the temperature of the gas increases, the pressure increases. Temperature and pressure are directly proportional.
• For example, http://www.marymount.k12.ny.us/marynet/06stwbwrk/06gas/1amcslussac/amcsgaylussac.ht
ml
Symbolic Representation of Gay Lussac’s Law
Pressure (kPa) • As temperature increases, pressure increases.
• So, P/T = constant Temperature (K)
P
1
T
1
P T
2 2
Gay Lussac’s Practice
• A sealed cylinder of gas contains nitrogen gas at 1,000 kPa and a temperature of 293K. When the cylinder is left in the sun, the temperature of the gas increases to 323K. What happens to the pressure in the cylinder?
Step #1: Qualitative Assessment of the Problem Step #2: Quantitative Assessment of the Problem
P
1
T
1
P T
2 2 1 , 000
kPa
293
K P
2 323
K
Combined Gas Law • Assume the number of gas molecules remains constant,
temperature
,
pressure
and
volume
related.
are
P
1
T V
1 1
P
2
V
2
T
2
Combined Gas Law Example • A sample of gas has a volume of 283 mL at 25 o C and 0.500 atm pressure. What is the volume at 100 o C and 1.00 atm?
P
1
V
1
T
1
P
2
V
2
T
2 V 2 = 177 mL
Avogadro’s Law If the temperature and pressure are constant,
as the number of particles of the gas increases, the volume increases
. Number of particles and volume are
directly
proportional.
Symbolic Representation of Avogadro’s Law
Volume (L) • As number of particles increases, volume increases.
Number of Particles • So, V/n = constant
V
1
n
1
V
2
n
2
Ideal Gas Law
• An
ideal gas
collisions
is defined as one in which all between atoms or molecules
are perfectly elastic
and in which there are
no intermolecular attractive forces.
• Think of a gas as a collection of perfectly hard spheres which collide but which otherwise do not interact with each other. Like Billiards!!
More about Ideal Gas Law
• An ideal gas can be characterized by three variables : absolute pressure (P), volume (V), and absolute temperature (T). • The relationship between them may be deduced from kinetic theory .
Exceptions to the Ideal Gas Law
• at
low temperatures
(close to 0 K) the gas molecules have less kinetic energy (move around less) so they
do
attract each other. • at
high pressures
(like many, many kPa) the gas molecules are forced closer together so that the volume of the gas molecules becomes significant compared to the volume the gas occupies.
Symbolic Representation Ideal Gas Law
PV = nRT
• n = number of moles • R = universal gas constant = 8.3145 J/mol*K • One mole of an ideal gas at STP ( S tandard T emperature and P ressure) occupies 22.4 L.
Ideal Gas Law Example
• What volume is needed to store 0.050 moles of helium gas at 202.6 kPa and 400 K? PV = nRT P = 202.6 kPa (202.6)(V) = (0.050)(8.314)(400) n = 0.050 mol T = 400K (202.6)(V) = 166.28
V = ? L R = 8.314 J/mol*K V=166.28/202.6
V = 0.821
Another Example
• What pressure will be exerted by 20.16 g hydrogen gas in a 7.5 L cylinder at 20 o C?
What are we trying to find?
Pressure!
Do we need to change any units?
Celsius
Kelvin
20 C + 273 = 293
Mass:
Grams
mass
moles = 20.16 g
molar mass of H 2
= 2 x 1.008 =2.016 g/mol
What do we know?
V= 7.5 L T= 20 Celsius R= 8.314 J/mol*K n= 20.16 g 20 .
16
g
1
mole
2 .
016
g
10
mol
NOW SOLVE!