All Flashcards
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.
Label the axes and curve in the following graph illustrating Boyle's Law.
X-axis: Volume (V), Y-axis: Pressure (P), Curve: Inverse relationship at constant temperature.
Label the axes and curve in the following graph illustrating Charles' Law.
X-axis: Temperature (T), Y-axis: Volume (V), Curve: Direct relationship at constant pressure.
What is the effect of increasing the temperature of a gas in a closed container with constant volume?
The pressure of the gas increases.
What happens to the volume of a gas if the pressure is decreased at a constant temperature?
The volume increases (Boyle's Law).
What happens if the number of moles of gas in a container increases, while volume and temperature are constant?
The pressure increases.
What is the effect of decreasing the temperature of a gas in a container at constant pressure?
The volume decreases (Charles' Law).