Unit 1 flashcards (Thermodynamics)

3 phases of matter

3 phases of matter

Solids, liquids, and solids

Solid

Crystalline structure, non-compressible

Liquid

no structure, but touching, non-compressible

Gas

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

Sublimation

Solid to gas

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. (Kind of temperature)

Temperature

the average measure of kinetic energy.

Kelvin

absolute zero (no zeros)

Endothermic

Absorbs heat

Exothermic

Releases heat

Heat of fusion

Solid ⇌ liquid (Melting point)

334 j/g

Heat of fusion for water (On reference table)

heat of vaporization

Liquid ⇌ Gas (Boiling point)

2260 j/g

Heat of vaporization for water (On reference table)

Specific heat capacity

there is a change in temp, but not phase.

4.18 j/gk

Specific Heat capacity of water (On reference table)

q=mHv

equation for heat of vaporization

q=mHf

equation for heat of fusion

q=mC∆T

equation for specific heat capacity

Properties of gasses

-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 pressure

Standard pressure

1 atm or 101.3 kPa or 760 torr

Standard temperature

0°C 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))

Combined gas Law equation

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

Uses for combined gas law

to find missing factors such as temperature, volume, or pressure, if one of those has also been changed.

KMT

Kinetic Molecular Theory

properties of KMT (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

gas that follows all rules in KMT

Real gas

gas molecules do have a volume and weak attractive forces

High temperature and low pressure

Conditions when Real gas acts most like Ideal gas

Vapor pressure

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

calorimetry

How to measure the amount of heat absorbed or released in a chemical reaction.

Specific Heat

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

Bromine and mercury

The two elements that are liquid at room temp

Iodine and Carbon Dioxide

The two elements that Sublimate at STP

Pressure increases

when volume decreases