What are the key differences between using $PV=nRT$ and $PV=NkT$?
$PV=nRT$: Uses number of moles (n) and the ideal gas constant (R). | $PV=NkT$: 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.
What are the key differences between using $$PV = nRT$$ and $$PV = Nk_BT$$?
$$PV = nRT$$: Uses number of moles (n) and the ideal gas constant (R). $$PV = Nk_BT$$: Uses number of molecules (N) and Boltzmann constant ($$k_B$$).
What are the differences between real gases and ideal gases?
Ideal Gases: Follow the ideal gas law perfectly, negligible intermolecular forces, point particles. Real Gases: Deviate from ideal behavior at high pressure/low temperature, significant intermolecular forces, finite particle volume.
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.
