States Of Matter Flashcards
What are the phases/states of matter
Solid, liquid, gaseous state
What are the differences between the 3 states of matter
Solid - strong cohesive forces, definite shape & volume, particles only vibrate
Liquid - less strong cohesive forces, definite volume, takes shape of container, particles slide over each other
Gases - negligible cohesive forces, indefinite volume & shape, particles move freely and randomly
What is sublimation
It is the change of state of a substance from solid to gas directly
State the names given to the conversion of each state of matter to another
Solid - liquid: melting/fusion
Solid - gas: sublimation
Liquid - solid: freezing
Liquid - gas: vapourization
Gas - solid: deposition
Gas - liquid: condensation
What is the temperature at which the saturated vapour pressure is equal to the atmospheric pressure called
Boiling point
When is the vapour pressure of a liquid saturated?
When the number of loquid molecules evaporating/vapourizing is equal to the number of vapour molecules condensing
Describe the change of atmospheric pressure with altitude
Atmospheric pressure reduces with increasing altitude and vice versa
Describe the change of boiling points with atmospheric pressure
As atmospheric pressure increases, the boiling point rises and vice versa
What is latent heat
It is the heat absorbed or released by a substance during a phase change without a change in temperature
During which phase changes is heat absorbed/gained
Melting, vapourization/boiling, sublimation
During which phase changes is heat released
Freezing, condensation, deposition
What are the phenomena that support kinetic theory of matter
Diffusion, osmosis, brownian motion
What are the assumptions of kinetic theory
- Gas particles are in constant rand motion in a straight line
- Their collisions are perfectly elastic
- Their collisions with the walls of the container results in pressure
- The volume fo gases are negligible when compared to the volume occupied
- The cohesive forces between gas particles are negligible
- Tbe temperature is a measure of the average kinetic energy of the particles
State Charles’s law
At constant pressure, the volume of a given mass of gas is directly proportional to the temperature
State dalton’s law of partial pressure
(1802)It states that when there is a mixture of gases which do not react chemically together, the total pressure of the system is the sum of the partial pressures of the individual elements
State Graham’s law of diffusion
(1833) It states that the rate of diffusion of a gas is inversely proportional to the square root of its density
What is the critical temperature of a gas
It is the temperature above which a gas cannot be liquefied by pressure
What is the critical pressure of a gas
It is the pressure at which the critical temperature is just enough to liquify the gas
State gay-lussac’s law of combining volumes
It states that when gases react, they do so in volumes which are simple ratios to one another and to the volumes of their products if gaseous provided that the temperature and pressure are kept constant
Mention some applications of Graham’s law
- it’s used to separate mixed gases(atmolysis)
- It’s used to determine density of gases
State avogadro’s hypothesis
It sates that equal volume of all the gases at the same temperature and pressure contain the same number of molecules
When do avogadro and Gay-lussac laws hold
At low pressures
What is the formula for calculating root mean square velocity
(3RT/m(in kg/mol))½
The velocities of gases are inversely proportional to the square root of their vapour densities.
True or false
True
What is the velocity of molecules of a gas given in terms of R, T and momentum(m)
c =(3RT/m)^½
At what conditions are gas laws obeyed more by gases
High temperatures and low pressures
What are the causes of the deviation from avogadro’s hypothesis and gay lussac’s law
The mutual attraction of molecules
The actual volume of the gas molecules
Do ideal gases condense
Gas laws do not account for condensation and believes that at 0K the volume of gases should be zero, but all gases condense before that temp.
