IDEAL Flashcards
What is an ideal gas?
An ideal gas is a theoretical gas composed of many randomly moving point particles that are not subject to interparticle interactions.
How do real gases differ from ideal gases?
Real gases have molecules with finite volume and experience intermolecular forces, while ideal gases are a simplification with negligible volume and no intermolecular forces.
Under what conditions do real gases behave like ideal gases?
Real gases behave most like ideal gases under low pressure and high temperature.
What happens to real gases at high pressure?
At high pressures, molecules are forced closer together, making their volume significant and increasing the effects of intermolecular forces.
What happens to real gases at low temperature?
At low temperatures, kinetic energy decreases, and intermolecular forces become more effective, potentially leading to condensation or solidification.
What are the limitations of the ideal gas model?
The ideal gas model does not account for the finite size of gas molecules, intermolecular forces, or phase transitions.
What is the ideal gas equation?
The ideal gas equation is PV = nRT.
What do the variables in the ideal gas equation represent?
P is pressure (Pa), V is volume (m³), n is amount of gas (mol), R is the ideal gas constant, and T is absolute temperature (K).
How can the ideal gas equation be expressed in terms of the number of molecules?
The ideal gas equation can be expressed as PV = Nk_B T.
What is the ideal gas constant (R)?
The ideal gas constant relates the energy scale to the temperature scale when dealing with moles of particles, approximately 8.31 J mol⁻¹ K⁻¹.
What is Boyle’s Law?
At constant temperature and number of moles, the pressure of a gas is inversely proportional to its volume (P ∝ 1/V).
What is Charles’s Law?
At constant pressure and number of moles, the volume of a gas is directly proportional to its absolute temperature (V ∝ T).
What is Gay-Lussac’s Law?
At constant volume and number of moles, the pressure of a gas is directly proportional to its absolute temperature (P ∝ T).
What is the kinetic theory of gases?
The kinetic theory of gases explains macroscopic properties of gases in terms of the motion of their constituent molecules.
How is pressure explained in the kinetic theory of gases?
Pressure is due to continuous collisions of gas molecules with the walls of their container.
What is the formula for root mean square speed (c_rms)?
c_rms = √(3PV / Nm).
How does temperature affect root mean square speed?
The root mean square speed is directly proportional to the square root of the absolute temperature (T).
What are the six assumptions of the kinetic theory of gases?
- Large number of molecules with large separation. 2. Continuous random motion. 3. Perfectly elastic collisions. 4. Negligible collision time. 5. No intermolecular forces except during collisions. 6. All molecules are identical.
