matter Flashcards
equation for specific heat capacity (c)? (E, m, θ)
ΔE = mcΔθ
where E = energy, m = mass and θ = change in temperature (IN KELVINS)
equation for change in momentum molecules experience when they hit side of container? (F, m, v, u, t)
F = (mv - mu)/Δt
equation for pressure (P)? (F, A)
P = F/A
where F = force and A = cross-sectional area
‘equation’ for distance (d) moved by particles in random walk (due to brownian motion)? (N)
d ∝ √N
where N = number of steps taken by particle
‘equation’ for distance (d) moved by particles in random walk (due to brownian motion)? (t)
d ∝ √t
t = time taken for particle to be displaced
equation for average KE of a particle? (m, <c^2>)
KE = 0.5m<c^2>
where m = mass and <c^2> = mean square speed (alternate symbol below)
average energy (E) of a particle? (T)
E = 1.5kT
where k = boltzmann’s constant and T = temperature in Kelvins
equation for root mean square speed (c rms)? (T, m)
c rms = √[(3kT)/m]
equation for total internal energy/KE of ideal gas (so all particles summed together)? (N, m, <c^2>)
E total = 0.5Nm<c^2>
where N = number of particles/molecules [NOT MOLES], m = mass and <c^2> = mean square speed
equation for charles’ law?
V ∝ T
OR
V/T = constant
[at constant pressure]
where V = volume and T = temperature
equation for pressure law?
p ∝ T
OR
p/T = constant
[at constant volume]
where p = pressure and T = temperature
equation for boyle’s law?
p ∝ 1/V
OR
pV = constant
[at constant temperature]
‘equation’ (the relationship) for density (ρ) of gas w fixed mass?
ρ ∝ 1/volume
so
ρ ∝ pressure
equation of state for gas?
pV/T = constant
OR
p1V1/T1 = p2V2/T2
ideal gas equation? (p, V, N, k, T)
pV = NkT
where p = pressure, V = volume, N = number of molecules/particles of gas, k = boltzmann constant
ideal gas equation (p, V, n, R, T)
pV = nRT
where p = pressure, V = volume, n = number of moles of gas, R = molar gas constant, T = temperature
equation for kinetic theory of gases? (p, V, N, m, <c^2>)
pV = (0.33…)Nm<c^2>
equation relating pressure (p), density (ρ) and mean square speed (<c^2>) of particles in gas?
p = (0.33…)ρ<c^2>
equation for density (ρ) of a gas? (N, m, V)
ρ = Nm/V
equation for APPROXIMATION of average energy (E) of particle? (T)
E ≈ kT
where k = boltzmann constant and T = temperature in Kelvins
how to work out if reaction will take place at noticeable rate? (ε, T)
ε/kT = constant
if ratio = 15 to 30, then reaction will take place at noticeable rate (bc some particles will always have above average energy)
(if above 30, reaction will be too slow to be noticeable, and if below 15, reaction will be too fast to be noticeable)
equation for how many particles have how many times more energy particle has above/below average particle energy?
n1E = N(f^n2)
where n1 = number of levels (i made up this constant), E = kT (energy gained/lost in each collision), N = total number of particles and n2 = number of successive collisions (i made up this constant)
n1 = n2
equation for the boltzmann factor (f) (aka, ratio of number of particles in two different energy states)? (ε, T)
f = e^(-ε/kT)
where ε = activation energy (i.e. energy of particles in higher energy state) and kT = average energy of particle
equation for number of particles that can go through with reaction (have higher energy state)? (
N = N0 x f
OR
N = N0[e^-ε/kT]
where N = number of particles that can go through with reaction (made up this constant), N0 = number of particles in whole sample (made up this constant), f = boltzmann constant
equation for total pressure (p) exerted by N molecules on side of container? (m, u, V)
p = (Nm<u^2>)/V
or
pV = (0.33…)Nm(c rms^2)
[look familiar?]
where N = number of particles/molecules, m = mass, <u^2> = mean square initial speed and V = volume
equation for number of molecules (N) contained in n moles of substance?
N = n x N A
where n = number of moles and N A = avogadro’s constant
equation for number of moles in substance of mass Ms of molar mass M?
n = Ms/M
