Leacture 1 Flashcards
What are the four measurable quantities of a gas?
Mass, pressure, volume, and temperature.
What does Boyle’s Law state?
At constant temperature, the pressure of a gas is inversely proportional to its volume (P ∝ 1/V).
What does Charles’s Law state?
At constant pressure, the volume of a gas is directly proportional to its temperature (V ∝ T).
What is the combined gas law formula for an ideal gas?
PV = nRT, where P is pressure, V is volume, n is moles of gas, R is the gas constant, and T is temperature.
Define Avogadro’s Law.
Equal volumes of all gases at the same temperature and pressure contain the same number of molecules.
What is Graham’s Law of Diffusion?
The rate of diffusion of a gas is inversely proportional to the square root of its molar mass.
What is the Kinetic Theory of Gases?
It describes gases as large assemblies of molecules with four key assumptions, including that gas molecules are in constant, random motion.
According to the Kinetic Theory, what does the mean kinetic energy of gas molecules depend on?
The temperature of the gas.
What is the root mean square velocity formula for gas molecules?
c^2^avg= 3RT/M where R is the gas constant, T is temperature, and M is the molar mass.
What are real gases, and how do they differ from ideal gases?
Real gases have intermolecular attractions and finite molecular volumes, leading to deviations from ideal behavior.
What is the Van der Waals equation for real gases?
𝑃+𝑎/(𝑉2)=𝑅𝑇, where a and b are constants that account for intermolecular forces and molecular volume.
How does the constant ‘a’ in the Van der Waals equation relate to intermolecular forces?
A higher value of ‘a’ indicates stronger intermolecular forces.
Define diffusion.
The tendency of molecules to spread out and move from areas of high concentration to areas of low concentration.
