Chemistry 3 final exam concepts set

What causes gas pressure

Collisions of gas particles with the walls of a container

What does Boyles Law describe

Pressure and volume are inversely proportional at constant temperature

What happens to volume when pressure increases`

Volume decreases

What does Charles law describe

Volume and temperature are directly proportional at constant pressure

What happens to gas volume when temperature increases

Volume increases

What is the Ideal Gas Law

PV=nRT

What does n represent in the Ideal Gas Law

the number of moles of gas

Daltons Law of Partial Pressures

Total pressure = the sum of all partial pressure

Particle speed as temperature increases (KMT)

Particle speed increases

Units for temperature in gas law calculations

Kelvin

Definition of IMFs

Attractions between molecules

Weakest Molecular Force

London Dispersion Forces

What moelcules experience dipole dipole forces

Polar molecules

What atoms allow for hydrogen bonding

FON

Definition of surface tension

The surface of a liquid will resist breaking

Definition of viscocity

Resistance to flow

How string IMFs affect boiling point

IMFs increase boiling point

How IMFs affect vapor pressure

Decrease vapor pressure

Phase change from liquid to gas

Vaporization

Phase change from gas to liquid

condensation

Phase change from solid to gas

sublimation

what phase change is gas to solid

deposition

effect on temperature during a phase change

Temperature will remain constant

Definition of a solute

the substance that is dissolved

definition of a solvent

The substance will dissolve another

like dissolves like

substances with similar polarity will dissolve eachother

Definition of a weak electrolyte

A substance that partially dissociates into ions

what is a strong electrolyte

a substance that completely dissolves into ions

What is a nonelectrolyte

a substance that does not produce ions in a solution

What is molarity

moles of solute per liter of solution

what is molarity

M = moles/lters

What is the affect of pressure on gas solubility

high pressure increases gas solubility

effect of temperature on gas solubility

higher temperature decreases gas solubility

what do colligative properties depend on

the number of dissolved particles

What are four colligative properties

Vapor pressur elowering, boiling point elevation, freezing point depression and osmotic pressure

what are chemical kinetica

the study of reaction rates

What is the definition of a reaction rate

the change in concentration over time

factors of increased reaction rate

higher concentration, higher temperature, lager surface area, catalysts

What does collision theory state

Particles must collide with sufficient energy and proper orientation to react

Definition of activation energy

the minimum energy needed for a reaction to occur

What effect does a catalyst have on activation energy

It lowers activation energy

Isa catalyst consumed during a reaction

No

What is a general rate law

Rate=k[A]^m[B]^n

How is the overall reaction order determined

add all exponents in the rate law

What is the first order half-life equation

t(0.5) = (0.693)/k

What graph gives a straight line for a first order reaction

Ln[A] vs time

Definition of dynamic equilibrium

Forward and reverse reactions occur at equal rates

At equilibrium, are concentrations equal?

Not necessarily; they are constant

Definition of the equlibrium constant

A ratio of product concentrations to reactant concentrations at equilibrium

What does a large K value indicate

Products are favored

What does a small K value indicate

Reactants are favored

Defintiion of reaction quotient

An equillibrium expression using current concentrations

If Q<K, which direction will the reaction shift

towards products (right)

If Q>K which direction will the reaction shift

towards reactants (left)

What is Le Chateliers Principle

A system at equilibrium shifts to oppose a stress

What happens if more reactant is added

Equilibrium shifts right

What happens if more product is added

Equilibrium shifts right

What happens if more product is added

Equilibrium shifts left

Increasing pressure favors which side of a gaseous equilibrium

the side with fewer moles of gasd

does a catalyst change the value of K

no