All Flashcards
Define the Ideal Gas Law.
The Ideal Gas Law describes the relationship between pressure (P), volume (V), number of moles (n), ideal gas constant (R), and temperature (T) of an ideal gas: or
What is an ideal gas?
A theoretical gas that obeys the ideal gas law. Its particles have negligible volume, experience no intermolecular forces, and undergo perfectly elastic collisions.
Define pressure (P) in the context of the Ideal Gas Law.
Force exerted per unit area by gas particles colliding with the walls of a container. Usually measured in Pascals (Pa) or atmospheres (atm).
Define volume (V) in the context of the Ideal Gas Law.
The amount of space occupied by the gas. Usually measured in cubic meters (m³) or liters (L).
Define absolute zero.
The theoretical temperature at which an ideal gas would have zero pressure and minimal kinetic energy. It is 0 Kelvin or -273.15°C.
What is the ideal gas constant (R)?
A physical constant that relates the energy scale to temperature scale, with a value of 8.314 J/mol·K.
What is the effect of increasing the temperature of a gas in a closed container (constant volume)?
The pressure of the gas increases.
What is the effect of decreasing the volume of a gas at constant temperature?
The pressure of the gas increases (Boyle's Law).
What is the effect of increasing the number of moles of gas in a container at constant volume and temperature?
The pressure of the gas increases.
What is the effect of increasing the temperature of a gas in a container with a movable piston (constant pressure)?
The volume of the gas increases (Charles' Law).
What happens when a real gas is compressed to a very high pressure?
It deviates significantly from ideal gas behavior due to increased intermolecular forces and non-negligible particle volume.
What are the key differences between using and ?
: Uses number of moles (n) and the ideal gas constant (R). | : Uses number of molecules (N) and the Boltzmann constant (k_B).
How do real gases differ from ideal gases?
Ideal Gases: Follow assumptions of negligible volume, no intermolecular forces, elastic collisions. | Real Gases: Deviate at high pressure/low temperature due to significant volume and intermolecular forces.
Compare Boyle's Law and Charles' Law.
Boyle's Law: P and V are inversely related at constant T. | Charles' Law: V and T are directly related at constant P.