Review of Gas Laws and Properties

These flashcards cover the fundamental concepts, laws, and properties of gases as discussed in the lecture notes.

What defines a gas in terms of molecule behavior?

Molecules are far apart and fill the available space.

List four important characteristics of gases.

1) Gases are highly compressible

2) Gases are thermally expandable

3) Gases have low viscosity

4) Most gases have low densities.

What device is used to measure atmospheric pressure?

Barometer.

What is the formula for atmospheric pressure?

Pressure = Force / Area.

What is Boyle's Law?

At constant temperature, pressure is inversely proportional to volume (P1V1 = P2V2).

What must temperatures be expressed in when using Charles' Law?

Kelvin.

State Amonton’s Law regarding temperature and pressure.

Temperature is directly related to pressure (T ∝ P).

What does Avogadro's Law state about volume and the amount of gas?

Volume is directly proportional to the number of moles of gas (V ∝ n).

What is the standard molar volume of a gas at standard conditions?

22.4 L.

What is the Ideal Gas Law?

PV = nRT.

If n and V are constant, what relationship describes pressure and temperature?

P1/T1 = P2/T2.

What is Dalton’s Law of Partial Pressures?

The total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas.

How is the root mean square speed (urms) of gas molecules calculated?

urms = √(3RT/M), where R is the gas constant and M is molar mass.

According to Graham's Law, how does the rate of effusion relate to molar mass?

The rate of effusion of a gas is inversely proportional to the square root of its molar mass.

What happens to the average speed of gas molecules as molecular mass increases?

The average molecular speed decreases.

Define diffusion in terms of gas behavior.

Diffusion is the mixing of one gas into another, where gas molecules collide and exchange energy.

What is a common unit of pressure equal to 760 mmHg?

1 atmosphere (atm).

What is the relationship between gaseous pressure and the number of gas molecules?

Pressure is a function of the number of gas molecules present and their average molecular speed.

State the postulates of the kinetic molecular theory of gases.

1) Gases behave like particles with mass but no volume.

2) Gas particles are in constant, random motion.

3) Collisions between particles are elastic.

What does it mean for gas collisions to be elastic?

The total kinetic energy remains the same before and after the collision.

How is density related to the Ideal Gas Law?

d = MP/RT, where d is density, M is molar mass, P is pressure, and T is temperature.