Chemistry Exam 3

Boyles law is pressure and volume is inversely proportional, True or False

True

Boyles law is also that volume and temperature are not inversely proportional, True or False

False, in Boyles Law volume and temperature are directly proportional

In Avogadro’s Law volume and number of moles are

Directly proportional

In Gay-Lussac Law pressure and temperature are

Directly proportional

What is the ideal gas law? Are the other gas laws direvied from the ideal gas law?

Yes, the ideal gas law is Gas molecules do not attract or repel each other, The particles themselves are considered infinitely small, taking up zero volume compared to the space they inhabit( no volume or intermolecular forces)

PV= nRT

P= pressure ( atm)

V= volume (L)

N= mol

R= universal gas constant

R = 0.08206> atm / 62.36> torr

Charles Law is temp and volume are

Directly proportional

What is the kinetic molecular theory?

• Constant Motion: Particles move rapidly and randomly.

• Negligible Volume: Gas particles are small, with vast empty space between them.

• No Intermolecular Forces: Particles do not attract or repel.

Elastic Collisions: Collisions conserve kinetic energy and momentum.

Temperature & Energy: kinetic energy is directly proportional to Kelvin/temperature

Explaining Gas Laws with Kinetic molecular theory

Boyles law: less space= more frequent collusions

Charles law: Increasing temperature increases particle kinetic energy (they move faster). To keep pressure constant, the particles must spread out, creating a larger volume so that the faster particles do not hit the walls more frequently. 

Gay-Lussc: high temp = Faster/Harder collisions

Avagrodo: Adding more particles (moles) to a container means more particles are hitting the walls. To keep the pressure the same, the volume must increase to reduce the collision frequency. 

Something you need to know when it comes to Kinetic molecular theory….

• The Velocity of gas particles are inversely proportional to square root of molecular weight.So, Heavier gas molecules move slower!

Explain velocity of gas particles distribution.( The Maxwell Boltzmann Curve)

gas molecules in a container do not all move at the same speed; instead, they have a wide range of speeds, with most particles moving near an average speed, while some move very fast and others very slow. 

This distribution is usually visualized as an asymmetric "bell curve" where the x-axis is molecular speed and the y-axis is the number of molecules. 

temp and mass dependent

Temp: As temperature increases, the average speed increases.

Mass: Lighter molecules (like Helium) move faster and have a broader distribution of speeds, while heavier molecules (like Xenon) move slower and have a narrower distribution, even at the same temperature.

Explain how temperature effects kinetic energy(the velocity of particles)

Higher temp makes gas particles move faster

Diffusion definition

The process where gas molecules spread out, moving from high to low concentration areas

Effusion definition

The process in which gas molecules escape from a container through a tiny hole into a evacuated space

What to know about the Rate of effusion/difussion and velocity

The rate of effusion and diffusion depend on molecular velocity, which is directly related to the gas's temperature and inversely related to its molar mass( temp and gas velocity directly proportional) lighter gas have a high rms velocities, lighter gases move faster

Graham’s Law:

The rate of effusion/diffusion is inversely proportional to the square root of the molar mass of gas

Memorize the Van der Waal equation

(P + n² a/ V² ) (V—nb) =nRT

Constants: a and b

A: intermolecular attraction

B: volume of gas molecules

At large volumes a and b are relatively small and van der Waal’s equation reduces to ideal gas law at high temp and low pressures

Conditions that cause deviations from ideality(real gases)

when these assumptions are not true: ideal gas particles are assumed to have no volume

• Ideal particles are assumed to have no interactions with each other

• At low temp and high pressures b/c molecules are forced closer together, making their finite volume significant and allowing intermolecular attractions to become influentia

Arrhenius definition of acid-base reactions

acid: H+ ions in aqueous solution

Base: OH- ions in aqueous solutions

Boyle’s Law equation

• P1V1=P2V2

Charles Law equation

V1 /T1 =V2 /T2

Gay Lusaac’s Law equation

P1 / T1 = P2 / T2

Avogadro’s Law

V1 / n1 = V2/n 2

Combined Gas Law

P1V1 / T1 = P2V1/T2

T is kelvin

Vander Waal’s equation

P+ a(n/V)² x (V-nb)=nRT

Bronstead-Lowry definition

Acid: H+ donor

Base: H+ acceptor

Lewis definition of acid-base reactions

Acid: e- pair acceptor

Base: e- pair donor

In determine which elements is oxidated and reduced reactions H2O is

0 charge

Sigma vs. pi bonds

Sigma overlap on line

Pi don’t overlap over line

Same phase ( + + / - - ) bonding

Not different phases (+ - / - +) anti bonding