(DONE) Lecture 17 Flashcards
What are the factors that determine physical state (3)?
- chemical identiy of matter
- temperature
- pressure
For solids, liquids, and gases compare their
- volume
- shape
- density
- compressibility
- thermal expansion
- volume: definite, definite, indefinite
- shape: definite, indefinite, indefinite
- density: high, middle, least
- compressibility: small, larger than solid, large
- thermal expansion: small, small, moderate
Explain the kinetic molecular theory (7)
- Matter is composed of small particles.
- The particles are in constant random motion
- The particles interact with each other
- have PE and KE
- The velocity and KE of the particles increase with temperature
- Energy is transferred by collisions among particles
- energy of a particle is continually changing
Explain the difference between potential energy and kinetic energy
- stored energy that matter possesses due to position, condition and/or composition; issa cohesive force
- energy matter possesses because of particle motion; issa disruptive force
In solids, liquids, and gasses, which dominates?: PE or KE?
- solid: PE
- liquid: PE only slightly
- gas: KE
Differentiate between an endothermic and exothermic process
Endothermic process: energy absorbed during a change of state/ chemical reaction
Exothermic process: energy is released during an exothermic process
What is a calorie?
Amount of energy to raise temperature of 1g of water by 1 degree
Differentiate between: specific heat and heat capacity
The heat required to raise the temperature of 1 gram of a substance (in a particular physical state) by 1 K (Kelvin) or 1 degree Celsius).
The amount of heat required to raise the temperature of a given amount of a substance (in a particular physical state) by one degree.
Draw and label (6) heat curve for heat added and heat lost
labels
- axis
- BPT
- MPT
- 5 stages and corresponding specific heat/ heat of ___
- all liquid
- all vapour
Differentiate between evaporation and vaporization
- an endothermic process where liquid → gas at temperatures BELOW the boiling point of the liquid
- happens at boiling point
Define vapour
Gaseous state of substance that exists at temp and pressure where substance is normally a liquid
Define vapour pressure
- the pressure of vapour in contact with its liquid or solid form
- a physical property that increases with increasing temperature
Define equilibrium
2 opposite processes taking place at equal rates (rate of liquid evaporation = rate of vapour condensing)
Define volatile
A substance that readily evaporates at room temperature and has a high vapour pressure is said to be volatile
Define boiling
When conversion from the liquid to the vapour state occurs within the body of the liquid through bubble formation
Define boiling point
the temperature at which the vapour pressure of the liquid is equal to the external atmospheric pressure
What is the difference between vapour and gas?
- gas is a definitive state of matter
- a vapour is something that exists in 2 states simultaneously (likely liquid and gas) and requires energy input to be created (ex: steam)