Gases Chapter 8 Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Low 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.1 Properties of Gases Goal: Describe the Kinetic Molecular Theory of Gases and the units of measurement used for gases. Gases
We are surrounded by gases, but we are often unaware of their presence.
Of the elements on the periodic table, only a handful
are gases at room temperature: H2, He, N2, O2, F2, Cl2, and the noble gases.
Other common gases are molecules with oxygen and
small nonmetals: CO, CO2, NO, NO2, SO2, SO3
Generally, molecules that are gases at room temperature have fewer than 5 atoms and are from the 1st and 2nd period. Gases
The behavior of gases is quite different from that of liquids and solids.
× Gas particles are far apart, whereas particle of both liquids an solids are held close together.
× A gas has no definite shape or volume and will completely fill any container.
× Because there are great distances between gas particles, a gas is less dense than a solid or liquid and easy to compress. Kinetic Molecular Theory of Gases
1. A gas consists of 2. The attractive 3. The actual volume small particles (atoms forces between the occupied by gas or molecules) that particles of a gas are molecules is move randomly with usually very small. extremely small high velocities. compared with the Gas particles are far volume that the gas Gas molecules apart and fil a occupies. moving in random container of any size directions at high and shape. The volume of the speeds cause a gas to gas is considered fill the entire volume equal to the volume of a container. of the container.
Most of the volume of a gas is empty space, which allows gases to be easily compressed. Kinetic Molecular Theory of Gases
4. Gas particles are in constant 5. The average kinetic energy of motion, moving rapidly in gas molecules is proportional to straight paths. the temperature in Kelvin.
When gas particles collide, they Gas molecules move faster as rebound and travel in new the temperature increases. directions. At higher temperatures, gas Every time they hit the walls of molecules hit the walls of the the container they exert container more often and with pressure. more force, producing higher pressures. An increase in the number or force of collisions against the walls of the container causes an increase in the pressure of the gas. Applications
The kinetic molecular theory helps explain everyday things:
Smells Explosions We can quickly smell Sometimes tires or gas- perfume when a bottle is filled containers explode opened across the room when temperatures are too because its particles move high. rapidly in all directions. From the KMT, we know At room temp, air molecules that gas particles move move at 1000 mph. faster when heated, hit the walls of a container with more force, and cause a buildup of pressure inside a container. When we talk about a gas, we describe it in terms of 4 properties: Pressure Volume Temperature Amount Pressure (P)
Gas molecules are Common units: extremely small and move × atmospheres (atm) rapidly. × mm of mercury When they hit the walls of (mmHg) a container, they exert pressure. × in of mercury (inHg)
If we heat the container, × Pascals (Pa) the molecules move faster and smash into the walls × torr more often and with increased force, thus × pounds per square increasing the pressure. inch (psi) Volume, Temperature, Amount
Volume (V) Temperature (T) Amount of gas (n)
The volume of a gas The temperature of The amount of gas equals the size of a gas is related to refers to the mass of the container in the kinetic energy of the gas present. which the gas is its particles. placed. Units: grams or Kinetic Energy – moles Units: L, mL energy of motion. As particles move (moles are used in faster, they equations) generate more kinetic energy in the form of heat.
Units: Kelvin (no negative numbers) 12 13 Convert 4820 mmHg to atmospheres. (1 atm = 760 mmHg) Convert 48 psi to torr (14.7 psi = 1 atm = 760 mmHg) Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Low 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.2 Pressure and Volume (Boyle’s Law)
Goal: Use the pressure-volume relationship (Boyle’s Law) to determine the final pressure or volume when the temperature and amount of gas are constant. Pressure and Volume Imagine that you can see air particles hitting the walls inside a bicycle tire pump.
What happens to the pressure inside the pump as you push down on the handle?
As the volume decreases, the air molecules are crowded together. More collisions occur with the walls, increasing the pressure. P and V – Inverse Relationship
⁓‒⁞ ⁗‒⁖⁗⁕⁗⁓⁗„‒⁗⁗‒⁛⁕⁗⁓⁗ ⁓‒⁞ ⁗‒⁛⁕⁗⁓⁗„‒⁗⁗‒⁖⁗⁕⁗⁓⁗
When a change in one property causes a change in another, the two properties are said to be related.
If the changes occur in opposite directions, the properties are inversely related.
The inverse relationship between P and V is known as Boyle’s Law. P and V – Boyle’s Law
Boyle’s Law: the volume (V) of a sample of a gas changes inversely with the pressure (P) of the gas as long as there is no change in the temperature (T) or amount of gas (n)
A result of Boyle’s Law is the equation:
P1V1 = P2V2
P1 = initial pressure P2 = final pressure
V1 = initial volume V2 = final volume The pressure inside a tire pump is 1.4 atm at 3.0 L. If the volume is decreased to 2.0 L, what is the new air pressure? A bubble of natural gas (CH4) has a volume of 45.0 mL at 1.60 atm of pressure when underground. What volume will the bubble have it if reaches Earth’s surface where atmospheric pressure is 744 mmHg? Assume no change in temperature or amount of gas. (760 mmHg = 1 atm) FYI – PV relationship in Breathing
The importance of Boyle’s Law is shown in the mechanics of breathing.
Our lungs are elastic, balloon-like structures contained in an airtight chamber called the thoracic cavity. The diaphragm, a muscle, forms the flexible floor of the cavity. FYI – PV relationship in Breathing
Inhalation (Inspiration) The process of taking a breath begins when the diaphragm contracts, causing an increase in the volume of the lungs. According to Boyle’s Law, this causes pressure in the lungs to decrease.
The pressure of the lungs drop below the atmospheric pressure creating a pressure gradient between the lungs and atmosphere.
Air molecules flow from higher pressure to lower and you breathe in. FYI – PV relationship in Breathing
Exhalation (Expiration) occurs when the diaphragm relaxes and moves back up into the thoracic cavity. The volume of the thoracic cavity and lungs decrease, causing an increase in the pressure in the lungs.
Now the pressure in the lungs in higher than the pressure of the atmosphere and a new pressure gradient causes the air molecules to flow out of the lungs. Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Low 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.3 Temperature and Volume (Charles’ Law)
Goal: Use the temperature-volume relationship (Charles’ Law) to determine the final temperature or volume when the pressure and amount of gas are constant. Hot air balloons…
You are going to take a ride in a hot air balloon. The captain turns on a propane burner to heat the air inside the balloon. As the air is heated, it expands and becomes less dense than the air outside, causing the balloon to rise… Charles’ Law
In 1787, Jacques Charles, a balloonist and physicist, proposed that the volume of a gas is directly related to temperature.
Charles’ Law: The volume (V) of a gas is directly related to the temperature (T) when there is no change in the pressure (P) or amount (n) of gas.
″‒⁗ ⁗⁓⁗‒⁛⁕⁗⁓⁗„‒⁞ ⁗‒⁛⁕⁗⁓⁗ ″‒⁗ ⁗⁓⁗‒⁖⁗⁕⁗⁓⁗„‒⁞ ⁗‒⁖⁗⁕⁗⁓⁗‒
29 Charles’ Law
= constant P and n
*Use Kelvins to avoid negative numbers.
30 A sample of helium gas has a volume of 5.40 L and a temperature of 15°C. What is the final volume, in liters, of the gas if the temperature has been increased to 42°C at constant pressure and amount of gas. Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Low 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.4 Temperature and Pressure (Gay-Lussac’s Law)
Goal: Use the temperature-pressure relationship (Gay- Lussac’s Law) to determine the final temperature or pressure when the volume and amount of gas are constant. If we could observe the molecules of a gas as the temperature rises, we would notice that they move faster and hit the sides of the container more often and with greater force.
If volume and the amount of gas are kept the same, we would see an increase of pressure.
34 Gay-Lussac’s Law
Gay-Lussac’s Law: the pressure of a gas is directly related to its Kelvin temperature at a constant volume and amount of gas
⁓‒⁗ ⁗⁓⁗‒⁛⁕⁗⁓⁗„‒⁗⁗‒⁛⁕⁗⁓⁗ ⁓‒⁗ ⁗⁓⁗‒⁖⁗⁕⁗⁓⁗„‒⁗⁗‒⁖⁗⁕⁗⁓⁗
= constant n and V
*All temperatures in Kelvin
35 An oxygen tank has a pressure of 120 atm at room temperature of 25.0°C. If a fire in the room causes the temperature of the gas in the tank to reach 402°C, what will be its pressure?
Tanks can rupture if pressure exceeds 180 atm. Will it explode? Vapor Pressure
When liquid molecules gain sufficient kinetic energy, they break way from the surface and become gas particles or vapor.
In an open container, all the liquid will eventually evaporate.
In a close container, the vapor accumulates above the liquid and creates pressure called vapor pressure.
37 Vapor Pressure
Each type of liquid exerts its own vapor pressure at a given temperature.
As the temperature increases, more vapor forms, and the vapor pressure increases. Boiling point
A liquid reaches its boiling point when its vapor pressure becomes equal to the external (atmospheric) pressure.
At high altitudes, where atmospheric pressure is lower, the vapor pressure to reach is lower, so water boils at a lower temperature!
Atmospheric Boiling point pressure of water Sea Level 760 mmHg 100°C
Denver 630 mmHg 95°C Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Law 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.5 The Combined Gas Law
Goal: Use the combined gas law to calculate the final V, P, or T of a gas when changes in 2 of these properties are given and the amount of gas is constant. Combined Gas Law
All of the Pressure-Volume-Temperature relationship for gases that we have studied may be combined into a single relationship called the Combined Gas Law:
= constant n Combined Gas Law
By using the combined gas law, we can derive any of the gas laws by emitting the properties that don’t change.
= constant n A 25 mL bubble is released from a diver’s air tank at a pressure of 4.00 atm and a temperature of 11°C. What is the volume, in mL, of the balloon when it reaches the ocean surface where the pressure is 1.00 atm and the temperature is 18°C? (Assume the amount of gas in the bubble does not change.) Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Law 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.6 Volume and Moles (Avogadro’s Law)
Goal: Use Avogadro’s Law to calculate the amount of volume of a gas when the pressure and temperature are constant. Up til now, we have always kept the amount of gas (n) constant. Now we will consider the affects when grams or moles change. WhenW you blow up a balloon, its volume increases becausese you add more air molecules.
If the balloon has a hole in it, air leaks out, causing its volume to decrease.
⁚⁗‒⁚⁗‒⁓ ‒⁘‒⁙⁓‒⁛⁕⁗⁓⁗„‒⁚⁗‒⁞ ⁗‒⁛⁕⁗⁓⁗ ⁚⁗‒⁚⁗‒⁓ ‒⁘‒⁙⁓‒⁖⁗⁕⁗⁓⁗„‒⁚⁗‒⁞ ⁗‒⁖⁗⁕⁗⁓⁗ Avogadro’s Law
In 1811, Amedeo Avogadro proposed:
Avogadro’s Law: The volume of a gas is directly related to the number of moles of a gas when T and P do not change.
For example, if the number of moles of gas doubles, then the volume will double too, as long as P and T do not change.
= constant P and T A weather balloon with a volume of 44 L is filled with 2.0 moles of He. What is the final volume if 3.0 moles are added for a total of 5.0 moles? (P and T don’t change.) Using Avogadro’s Law, we can say any two gases will have equal volumes if they contain the same number of moles of gas (at the same T and P). STP Standard Temperature and Pressure “STP” is a handy abbreviation for 373K (O°C) and 1 atm. A common set of units.
At STP, one mole of any gas occupies a volume of 22.4 L (roughly the volume of the 3 basketballs). Molar Volume The volume, 22.4 L, of any gas at STP is called its molar volume.
When a gas is at STP conditions (OC and 1 atm), its molar volume can be used as a conversion factor between # of moles and volume:
1 22.4 What is the volume, in liters, in 64.0 g of O2 gas at STP? Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Law 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.7 The Ideal Gas Law
Goal: Use the ideal gas law equation to solve for P, V, T, or n of a gas when given 3 of the 4 values in the ideal gas law equation. Calculate the mass or volume of a gas in a chemical reaction. Ideal Gas Law
The ideal gas law is the combination of the 4 properties used to measure gases - P, V, T, n – to give a single equation:
= Ideal Gas Constant =
N2O is an anesthetic (laughing gas). What is the pressure, in atm, of 0.350 mole of N2O at 22°C in a 5.00 L container? Often we need to know the amount of gas (in grams) involved in a reaction.
Then the Ideal Gas Law can be rearranged to solve for moles (n) then convert to grams using molar mass.
61 Butane, C4H10, is used as a fuel for camp stoves. If you have 108 mL of butane gas at 715 mmHg and 25°C, what is the mass, in grams, of butane. Gas Laws and Chemical Reactions
Gases are involved as reactants and products in many chemical reactions. Typically the information given for a gas is its P, V, and T. Then we can use the ideal gas law to determine the moles of a gas in a reaction.
If we know the number of moles for one of the gases, we can use mole-mole factors to determine the moles of any other substance.
63 Calcium carbonate (CaCO3) in antacids reacts with HCl in the stomach to reduce acid reflux. How many L of CO2 are produced at 752 mmHg and 24°C from a 25.0 g sample of calcium carbonate.
CaCO3(s) + 2HCl(aq) Æ CO2(g) + H2O(l) + CaCl2(aq) Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Law 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law) 8.8 Partial Pressures (Dalton’s Law)
Goal: Use Dalton’s Law of partial pressures to calculate the total pressure of a mixture of gases. Gas Mixtures
Many gas samples are a mixture of gases.
For example : the air we breathe is a mix of mainly nitrogen and oxygen.
In gas mixtures, scientists observed that all gas particles behave in the same way.
Therefore the total pressure of the gases in a mixture is a result of the collisions of the gas particles regardless of what type of gas they are.
67 Dalton’s Law
In a gas mixture, each gas exerts its partial pressure (the pressure it would exert if it were the only gas in the container).
Dalton’s Law states that the total pressure of a gas is the sum of the partial pressures of the gases in the mixture.
Ptotal = P1 + P2 + P3 + …
68 Example
If we combine the gases into one tank, with the same V and T, the number of gas molecules (n) determine the pressure of the tank.
It does not matter what type of gas (He or Ar). Simply how many atoms of gas there are. 69 A heliox breathing mixture of oxygen and helium is prepared for a patient. The gas mixture has a total pressure of 7.00 atm. If the partial pressure of the oxygen is 114 mmHg, what is the partial pressure of the helium? Chapter 8
8.1 - Properties of Gases 8.2 – Pressure and Volume (Boyle’s Law) 8.3 – Temperature and Volume (Charles’ Law) 8.4 – Temperature and Pressure (Guy-Lussac’s Law) 8.5 – The Combined Gas Law 8.6 – Volume and Moles (Avogadro’s Law) 8.7 – The Ideal Gas Law 8.8 – Partial Pressures (Dalton’s Law)