gas laws

i almost saw god this week cut me some slack on being late

what state of matter has the highest kinetic molecular energy

gas (solids have the lowest)

What is kinetic molecular theory?

* It explains the behavior of the phases of matter in terms of the motion of particles 
* This is like saying solids have a fixed shape and volume because their particles don’t have any motion 

what does kmt explain

the properties of gases, particularly ideal gases

what are ideal gases in this context

Ideal gases do not exist in nature, but many real gases have properties similar to Ideal Gases under certain conditions 

what are the 5 postulates of ideal gases

motion of gas particles is linear

Collision between gas particles are elastic

No intermolecular attraction between gas particles

Gas particles have no volume

Temperature is a measure of average kinetic energy of the gas particles

motion of gas particles is linear (explanation)

Particles are in continuous, random motion. Particles move in straight lines (linear), until they collide with something

Collision between gas particles are elastic (explanation)

* Collisions between gas particles and between the walls their containers are elastic collisions.
* This means there is no loss of kinetic energy during collisions. 

result of collisions between gas particles

This causes pressure to form! The more collisions there are, the more pressure there is.

No intermolecular attraction between gas particles (explanation)

There are no forces of attraction or repulsion between gas particles. This means that ideal gases have such small attraction to each other, it can be ignored

Gas particles have no volume (explanation)

* Gas molecules clearly have both mass and volume
* The volume of each molecule is so small, however, that each gas molecule is said to be a point without volume.
* The whole gas occupies the space available, but the volume taken by the individual particles is ignored.
* Gas particles are therefore, very far apart compared to the size of the individual gas particles

Temperature is a measure of average kinetic energy of the gas particles (explanation)

* The warmer gases have higher kinetic energy compared to colder gases.

When do Real Gases behave like ideal gases?

They behave like real gases when they are small, at high temperatures/greater temperatures, and pressure is low

temp (as a property of gas)

Temperature is defined as the **average kinetic energy** of the molecules of the gas.

\-measured in kelvins like from the office lol

how to measure kinetic energy (god physics i hate physics)

Since all of the molecules are in linear motion, and therefore have a velocity, they possess kinetic energy as defined by the following equation:

Kinetic Energy = ½ (mass)(velocity)2

KE = ½ mv^2

volume as a property of gas

* Volume is defined as the space that matter occupies.
* We always measure in liters

Pressure (as a prop of gas)

* Pressure is defined as the amount of force applied to an area of matter:

Pressure = Force / Area

pressure relationships

The area involved with pressure is the surface area of the container

As Force ↑, Pressure ↑

As Surface Area ↓, Pressure ↑

where does pressure come from

Gas particles apply force on the container as particles collide with the boundary

or

that one bands debut album

what do gas laws do

explain the relationships between pressure, volume, and temperature

Boyle’s Law

* Boyle’s Law states that at a **constant temperature (unchanging)**, the **volume** of a gas is **inversely** proportional to the **pressure**
* This means as the gas volume increases, the pressure would decrease.

reasoning behind boyles law

This is because as volume decreases, there is less space for the particles, causing more collisions, which makes pressure increase

charles law

* Charles’ Law states that at a **constant pressure**, the **volume** of a gas is directly **proportional** to the **temperature.**
* This means if the temperature of a gas increases, the volume increases as well 

reasoning behind charles law

this is because as a gas is heated up, the kinetic energy is increases, causing more collisions. The container (volume) will expand to maintain the same pressure

Gay-Lussac’s Law (i giggled ur lying if u didn’t giggle)

* gay-Lussac’s Law states that a **constant volume** the **pressure** of a gas is **directly proportional** to the **temperature** 
* This means as temperature increases, the pressure will also increase 

reasoning behind gay lussac’s law

This is because as temperature is increased, the kinetic energy is increased. More collisions occur because of this, so the pressure increases as well

boyles law is the math relationship between

pressure and volume (pv so inverse relationship)

charles law is the math relationship between

volume and temp (v/t so direct relationship)

gay lussac’s law is the math relationship between

pressure and temp (p/t so direct)

what is the combined gas law

(pv)/t

JOHN DALTON IS BACK in the law of partial pressure which is…

This law states that the **total pressure** experienced by a container containing more than one form of gas is the **sum of the pressures of each individual gas**.

what is the context for the law of partial pressure/why does it matter

* A single container can, and normally does, contain more than one type of gas.

**John Dalton**, attempting to describe the pressure exerted by each individual gas on the container, developed what is now called the **Law of Partial Pressure**.

Example-Gas collection over water (law of partial pressure)

One of the most common ways of collecting a gas sample is by having it buble into a jar filled with water. The collected gas is a mixture of the gas plus the water vapor. The amount of water vapor is very sensitive to temperature. 

how to solve the ex of gas collection over water

1. Get the vapor pressure of the water from a chart 
2. Subtract the vapor pressure from the total pressure of the system to get the pressure of the dry gas. 

ideal gas law is..

* This law is an equation of state for a hypothetical ideal gas
* It is a combination of Boyle's, Charles's, and Avogadro’s laws.
* pv=nrt

is the ideal gas law always exact

no, it is a good approximation to the behavior of many gases under many conditions, although it has several limitations (she did not enlighten us on said limitations so like just like know i guess)

what is the gas constant

* The Ideal Gas Constant is a set of values for standard conditions that we assume ideal gases to be at 
* Using those standard conditions, we are given a constant depending on the measurement of pressure used
* R = .0821 atm, 8.31 kPa, 62.4 mmHg

constant temp = constant

energy