Unit 1- Thermodynamics

Density

________- how closely packed matter is in a given volume.

Particles

________ are traveling in straight- line paths and are randomly distributed.

Liquid

________- no structure, but touching, non- compressible.

Temp

________ is the average measure of kinetic energy.

Kelvin

________- absolute zero (no zeros)

low temperatures

Can be liquified at ________ and high pressures.

Food labels

________ are actually kilocalories.

vapor pressure

A liquid will boil when its ________ equals the pressure of the liquid above it.

Vapor pressure

________ has a greater influence on boiling than temperature.

Kind of but not really)

energy of the motion of particles

Kelvin

absolute zero (no zeros)

conversion

K= c + 273

Endothermic

Absorb heat

Exothermic

release heat

equation for Heat of fusion

q=mHf

equation for Heat of Vaporization

q=mHv

equation for specific heat capacity

q=mCAT

Pressure

1 atm or 101.3 kPa or 760 torr

Temperature

0 C or 273 K

equation

V1/T1 = V2/T2

Formula(On back of reference table)

(P1)(V1)/T1 = (P2)(V2)/T2

Ideal Gas

Follows all rules above for gas

Real Gas

gas molecules do have a volume and weak attractive forces

Sublimation

Solid to gas

3 phases of matter

Solids, liquids, and gasses

Solids

Crystalline structure, non-compressible

Liquids

no structure, but touching, non-compressible

Gasses

No structure, spread out, compressible.

Physical properties

Properties that can be used to identify the substance(element)

Melting point

point when a solid becomes a liquid

Boiling point(vaporization)

point when a liquid becomes a gas

Freezing point(solidification)

point when a liquid becomes a solid

Density

how closely packed matter is in a given volume

Atomic Radius

refers to the space a specific element occupies.

potential energy

stored energy

Kinetic energy

energy of the motion of particles

Temperature

the average measure of kinetic energy

Kelvin

Absolute zero (No zeros)

Endothermic

absorb heat

Exothermic

release heat

334 j/g

energy for heat of fusion for water

2260 j/g

energy for heat of vaporization for water

4.18 j/gk

energy for specific heat capacity of water

q=mHf

equation for heat of fusion

q=mHv

equation for heat of vaporization

q=mCAT

equation for specific heat capacity

heat of vaporization

liquid to gas/ gas to liquid

heat of fusion

Solid to liquid/ liquid to solid

Specific heat capacity

change in temp, but not phase.

properties of gas

Particles are traveling in straight-line paths and are randomly distributed, No definite shape or volume, Large distances between particles, low densities, Can be compressed, Can be liquified at low temperatures and high pressures.

STP

standard temperature and pressure

Standard pressure

1 atm or 101.3 kPa or 760 torr

Standard temperature

0 C or 273 K

Boyle's Law

relationship between pressure and volume (says that the volume occupied by a gas is inversely proportional to the pressure exerted on the gas)

Charles's Law

Describes the relationship between volume and temperature (Says that the volume occupied by a gas is directly proportional to the temperature(in kelvin))

KMT

Kinetic Molecular Theory

properties of KMT (for Ideal gas)

gases move in a random, constant, straight line motion, Have negligible volume, no attraction between particles, If gas molecules do collide no energy is lost or gained.

Ideal gas

Follows rules from KMT

Real gas

gas molecules do have a volume and weak attractive forces

Real gas acts like Ideal gas

when there is a high temp and low pressure

Vapor pressure

The pressure that vapor exerts when the temperature of a liquid increases.

Specific heat

the heat required to increase the temperature of a substance by 1 degree

Bromium and mercury

The two elements which are liquid at room temp

Iodine and Carbon Dioxide

The two elements that sublimate at STP

Sublimation

Solid to gas/ gas to solid

pressure decreases

when volume increases