#5.1.4a
amount of substance in moles; Avogadro constant NA equals 6.02 × 1023 mol–1
#5.1.4b
model of kinetic theory of gases
Assumptions for the model:
- large number of molecules in random, rapid motion
- particles (atoms or molecules) occupy negligible volume compared to the volume of gas
- all collisions are perfectly elastic and the time of the collisions is negligible compared to the time between collisions
- negligible forces between particles except during collision
#5.1.4c
pressure in terms of this model
#5.1.4d
(i) the equation of state of an ideal gas \(pV = nRT\), where n is the number of moles
(ii) techniques and procedures used to investigate \(PV = \text{constant} \) (Boyle’s law)
and \(\dfrac{P}{T} = \text{constant} \)
PAG8
(iii) an estimation of absolute zero using variation of gas temperature with pressure
PAG8
#5.1.4e
the equation \(pV = \dfrac{1}{3} Nm\bar{c}^2 \),
where N is the number of particles (atoms or molecules) and \(\bar{c}^2\) is the mean square speed
Derivation of this equation is not required.
#5.1.4f
root mean square (r.m.s.) speed; mean square speed
Learners should know about the general characteristics of the Maxwell-Boltzmann distribution.
#5.1.4g
the Boltzmann constant; \(k = \dfrac{R}{N_A} \)
#5.1.4h
\(pV = NkT \);
\(\dfrac{1}{2}m\bar{c}^2= \dfrac{3}{2}kT \)
Learners will also be expected to know the derivation of the equation \(\dfrac{1}{2}m\bar{c}^2= \dfrac{3}{2}kT \) from \(pV = \dfrac{1}{3} Nm\bar{c}^2 \) and \(pV = NkT \)
#5.1.4i
internal energy of an ideal gas.