CH 301 Unit 3 Exam 1 Review Notes

These flashcards cover key concepts from the chemistry lecture notes for CH 301, focusing on gas laws, state functions, kinetic molecular theory, and related calculations.

What is the equation for the relationship of universe in chemistry?

Universe = system + surroundings.

What are state functions in chemistry?

Variables that define how a system ends from how it starts, e.g., ΔV, ΔT, Δn.

Provide examples of extensive and intensive properties.

Extensive: volume, mass; Intensive: temperature, density.

What are the five statements of Kinetic Molecular Theory (KMT)?

1. All gases are simple hard spheres.

2. All gases are infinitely small compared to V(system).

3. Gases have elastic collisions, so no energy change.

4. T increases, KE increases.

5. KE α (mν²); mass is inversely related to velocity.

What happens to gas velocity distributions at high and low temperatures?

At high temperature, the distribution broadens; at low temperature, it compresses.

What is Graham's law, and how does it relate to gas speeds?

The ratio of the rate of effusion of two gases is inversely proportional to the square root of their molar masses.

State Boyle's Law.

P1V1 = P2V2; it describes the inverse relationship of pressure and volume.

What is Dalton's Law in relation to gas mixtures?

The total pressure is the sum of the partial pressures of individual gases in the mixture.

Define the combined gas law equation.

P1V1/T1 = P2V2/T2; it relates pressure, volume, and temperature of a gas.

What is the Ideal Gas Law?

PV = nRT, where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature.

What corrections are made in the Van der Waals equation?

(P + a)(V + b) = nRT; 'a' corrects for intermolecular attractions, 'b' corrects for the volume occupied by gas molecules.

What is a characteristic of ideal gases regarding conditions?

Ideal gases behave best under conditions of low pressure and high temperature, where collisions are rare.

What is the relationship between molecular weight and density in the ideal gas law?

Density (ρ) increases as pressure (P) increases and molecular weight (MW) increases, and decreases as temperature (T) increases.