,Converting from Celsius (c) to Kelvin (k):
0 degrees Celsius = 273.15 Kelvins 0 Kelvins = - 273.15
Kelvins
Formula:
°C + 273.15 = K K - 273.15 = °C
Physical characteristics of Gases
It takes the shape of the container and assumes the volume
It is the most compressible state of matter
It mixes evenly and entirely when confined to the same container
It has a lower density than liquids and solids
How is the pressure of the gas caused?
It is caused by collisions, which is the momentum transfer of the molecules of the
gas with walls of the container.
What affects the frequency of the collisions?
The size of the pressure is impacts to how often the molecules hit the wall of the
container.
Pistons
The increase of temperature, cause more kinetic energy hence the molecules
are more energetic, therefore more collisions occur between the molecules
and the walls.
Increasing the temperature will increase the pressure
Decreasing the volume will reduce the frequency of the collisions, increasing
the pressure
When gas is heated using spark plugs it expand, confining the gas, hence
increasing the pressure.
The pressure will them exert a force on the surface of the piston, causing it
to move.
, Ideal Gas Law
A gas constant will change when dealing with different units of pressure and
volume
An ideal gas will behave as expected based on the assumptions of kinetic
theory.
Formula
PV = Number pf particles in gas X Boltzmann constant (1.3807 x 10 ) X Temperature
-23
PV = N X k X T
R
The pressure laws (Pressure vs Temperature)
Temperature is directly proportional to pressure, e.g., Temperature
increases, Pressure increases.
As the temperature of a gas increase, the pressure will increase as well.
The gas is heated > The particles will move faster colliding more frequently
with the walls of the container > a great force is exerted onto the walls > Volume
remains the same > Pressure increases
Formula
K = Pressure (P) / Temperature (T)
Boyles’s law (Pressure vs Volume)
0 degrees Celsius = 273.15 Kelvins 0 Kelvins = - 273.15
Kelvins
Formula:
°C + 273.15 = K K - 273.15 = °C
Physical characteristics of Gases
It takes the shape of the container and assumes the volume
It is the most compressible state of matter
It mixes evenly and entirely when confined to the same container
It has a lower density than liquids and solids
How is the pressure of the gas caused?
It is caused by collisions, which is the momentum transfer of the molecules of the
gas with walls of the container.
What affects the frequency of the collisions?
The size of the pressure is impacts to how often the molecules hit the wall of the
container.
Pistons
The increase of temperature, cause more kinetic energy hence the molecules
are more energetic, therefore more collisions occur between the molecules
and the walls.
Increasing the temperature will increase the pressure
Decreasing the volume will reduce the frequency of the collisions, increasing
the pressure
When gas is heated using spark plugs it expand, confining the gas, hence
increasing the pressure.
The pressure will them exert a force on the surface of the piston, causing it
to move.
, Ideal Gas Law
A gas constant will change when dealing with different units of pressure and
volume
An ideal gas will behave as expected based on the assumptions of kinetic
theory.
Formula
PV = Number pf particles in gas X Boltzmann constant (1.3807 x 10 ) X Temperature
-23
PV = N X k X T
R
The pressure laws (Pressure vs Temperature)
Temperature is directly proportional to pressure, e.g., Temperature
increases, Pressure increases.
As the temperature of a gas increase, the pressure will increase as well.
The gas is heated > The particles will move faster colliding more frequently
with the walls of the container > a great force is exerted onto the walls > Volume
remains the same > Pressure increases
Formula
K = Pressure (P) / Temperature (T)
Boyles’s law (Pressure vs Volume)
