ch 15 Flashcards
definition of a mole
the amount of substance which contains 6.022*10^23 elementary entities, such as atoms or molecules (could also be ions or electrons) //// amount of substance containing the same number of particles as in 0.012 kg of carbon-12
Avogadro constant NA
the number of elementary entities in 1 mole of any substance /// number of atoms of carbon-12 in 0.012 of carbon-12
boyle’s law
law stating that for a given mass of a gas, the volume of the gas is inversely proportional to its pressure, provided that the temperature is constant
charle’s law
volume of an ideal gas at constant pressure is directly proportional to the absolute temperature: V1/T1=V2/T2
ideal gas
gas that obeys the equation pV∝T at all pressures p, volumes V and thermodynamics temperature T at all values of pvt
gay-lussac’s law/ law of pressures
the relation between the pressure and thermodynamic temperature of a fixed mass of a gas at constant volume: p1/T1=p2/T2
equation of ideal gas
pV= nRT //// pV=NkT
equation of k
k=R/NA
The assumptions of the kinetic theory of an ideal gas
- All molecules behave as identical, hard, perfectly elastic spheres
- The volume of the molecules is negligible compared with the volume of the containing vessel
- There are no forces of attraction or repulsion between molecules
- There are many molecules, all moving randomly
force in kinetic theory
Δp/t where t=2L/cx ,,,,, mcx^2/L
Δof momentum
mcx-m-cx== 2mcx
what is Pythagoras’ theorem to three dimensions that gives the relation between c and the three components of velocity cx, cy and cz
c^2=cx^2+cy^2+cz^2
root-mean-square speed or r.m.s. speed
√<c2> = √ (3kT/ m)</c2>
what is <C^2>
the mean value of the square of the speeds/ velocities of the molecules
