Chemistry gas law

what temperature unit must be united when calculating gas

Kelvin

How do get from celsius to kelvin

add 273

what are pressure units

pascals (Pa), atmospheres (atm), torr, and millimeters of mercury (mmHg)

Boyles law

states that for a fixed amount of gas at a constant temperature, volume and pressure have an inverse relationship. Simply put: if you squeeze a gas (decrease volume), its pressure goes up; if you let it expand (increase volume), its pressure goes down

Boyle's Law equation

P₁V₁=P₂V₂

Charles's Law

if pressure is held constant, the volume of a gas increases as its temperature rises and decreases as its temperature falls

Charles's Law equation

V₁/T₁=V₂/T₂

Gay-Lussac's Law

states that for a fixed amount of gas in a rigid, non-changing container, pressure (\(P\)) is directly proportional to temperature (\(T\)). As temperature increases, gas molecules move faster and collide harder, raising the pressure. Conversely, if temperature drops, pressure decreases

Gay-Lussac's Law equation

P₁/T₁=P₂/T₂

Is Boyles an inverse relationship

yes as one goes up the other goes down

what combines Boyle's, Charles's, and Gay-Lussac's Lawsv

The combined gas law

Combined Gas Law equation

P₁V₁/T₁=P₂V₂/T₂

Dalton's Law

the total pressure of a non-reacting gas mixture is equal to the sum of the individual pressures (partial pressures) of each gas in the mixture.

Daltons law equation

Ptotal = P₁+P₂+P₃...

Ideal Gas Law

PV = nRT

True or False: Gas particles are so small they have no mass.

While particles are extremely small, they still have a defined mass.

How is the volume of individual gas particles described in an ideal gas model?

The volume is assumed to be zero (negligible) because it is so small compared to the total volume of the container.

What does it mean for gas particle collisions to be "perfectly elastic"?

There is no net loss or gain of kinetic energy during the collision; energy is simply transferred between particles or the container walls.

What factor determines the average kinetic energy of gas particles?

The temperature of the gas. Average kinetic energy is directly proportional to the absolute (Kelvin) temperature

Do gas particles attract or repel each other in the kinetic molecular theory?

No. It is assumed that gas particles exert no attractive or repulsive forces on one another

Amount of gas (n)

moles

Volume (V)

liters

Temperature (T)

In Kelvin for calculations

Pressure (P)

in atmospheres

How do we measure pressure

barometer and manometer

pressure conversion

1 atm = 760 torr = 760 mm Hg = 101,325 Pa= 101.3kpa

Standard Temperature and Pressure

STP is 1 atm and 273 K, which is O ºC)

Who studied the relationship between the pressure and volume of a gas while keeping temperature constant?

Robert Boyle

In Boyle's Law (P1V1=P2V2) what is the relationship between Pressure (p) and Volume (V)

They are inversely proportional (as one increases, the other decrease

What variable must remain constant for the equation (P1V1 = P2V2) to be valid?

Temperature (t) and the amount of gas (n)

How are volume (\(V\)) and temperature (\(T\)) related when pressure is held constant?

They are directly proportional. As the temperature of a gas increases, its volume increases, provided the pressure remains unchanged.

Who proposed that equal volumes of gases at the same temperature and pressure contain the same number of molecules/particles?

Amedeo Avogadro

What is the relationship between volume (v) and the number of moles (n) in Avogadro's Law (V=an)

Directly related

k/a

constant

Under what conditions is Avogadro's Law (V=an) valid?

At constant temperature and pressure

Gas Effusion

the process where gas molecules escape from a container into a vacuum or lower-pressure area through a tiny pinhole, with the rate determined by molecular mass and speed