the particulate nature of matter - whole of B

kinetic theory of matter

all matter is made up of atoms and molecules which are in perpetual motion

evidence for the kinetic theory of matter

brownian motion (random motion), diffusion (collision between particles)

conversion from celsius to kelvin

celsius + 273

conversion from kelvin to celsius

kelvin - 273

conduction

fast moving particles transfer KE to slower particles when they collide

convection

occurs due to variations in density of liquids and gases

radiation

transfer of thermal energy as an electromagnetic wave

gases in atmosphere that absorb IR

H20, CO2, N2O, CH4 → have resonant frequencies in the IR region which causes them to absorb and re-emit radiation in random directions

intensity is indirectly proportional to

r²

specific latent heat

the energy required to change the phase of 1 kg of a substace without a change in temperature

characteristics of an ideal gas

gas particles are spherical; collisions are perfectly elastic; no intermolecular PE stored between particles; total volume of gas particles is negligible in comparison to the volume of the container; monatomic gas

the mole

a mole of a substance contains the same number of elementary entities as the number of atoms found in 12g of carbon-12

boyle’s law

pressure is indirectly proportional to volume

pressure law

pressure is directly proportional to temperature

charles’ law

volume is directly proportional to temperature

isobaric change

constant pressure; change in temperature; Q = ΔU + PΔV

isovolumetric change

constant volume; change in temperature; no work done → Q = ΔU

isothermal change

constant temperature; no change in internal energy → Q = W

adiabatic change

no (heat) energy lost or gained; ΔU = W when work is done by the system; ΔU = -W when work is done on the system

in the first law of thermodynamics work is positive when

net work is done BY the system

cyclic process

a series of stages which returns a system back to its original state

carnot cycle

Consists of two isothermal transformations where heat is exchanged at the same temperature as the surroundings, and two adiabatic processes where no energy is exchanged with the surroundings

the clausius statement

energy cannot be transferred from a lower temperature body to a higher temperature body without work being done

the kelvin-planck statement

energy cannot be extracted from a hot body and transferred entirely into work

entropy

total “disorder” of a system; during irreversible changes entropy always increases