All equations Flashcards
SN2 rate equation
Rate= K [R-Hal][Nu]
SN1 rate equation
Rate= K[R-Hal]
Total internal energy of a system
U= W + q
Kinetic energy
Ekin= 1/2 mV2
work
w = f x d
Newtons law of force
F = m x a
Coulombs law
F = Kq1q2 / r2
energy
E = P x V
Change in enthalpy
∆H = ∆U + p∆V
entropy
S= KB ln (omega)
Change in entropy
-∆S= ∆H / T
spontaneous reaction with entropy
∆Stotal = ∆Ssystem + ∆Ssurroundings >0
Gibbs free energy
∆G = ∆H - T∆S
Probability of number of particles in a system
P (N, NL) = N! / (N - NL)! x 0.5N
spontaneous reaction with free energy
∆Gtotal = ∆Gproducts - ∆Greactants <0
Kc
Q
Van’t Hoff isotherm
∆G0 = - RT ln K
K = e(∆G^0 / RT)
∆G
∆G = - nfe
the two versions of the Nernst equation
E= Eø - (RT/ nF) ln Q (Q= [red]/[ox])
E= Eø + (RT/nF) ln Q (Q= [ox]/[red])
equations relating pH and H+
PH= -log10[H+]
H+= 10-pH
Nernst equation generalising the pH effect
E = (RTV/nF) x (-pH)
Rate of collision
πr2VR[A][B]
collision theory law and constant
Rate= K [A][B]
K= πr2VRe(-Ea/ RT)
The differential law for zero, first and second order reactions
Zero: rate = K
first: rate = K[A]
second: rate= K[A]2
The integrated rate equation for zero, first and second order reactions
Zero: [A]t = [A]0 - kt
first: [A]t = [A]0 e-kt
second: [A]t = [A]0 / 1 + kt [A]0
First order half life
t1/2 = ln 2 / k
Arrhenius equation (both versions)
K= Ae(-Ea /RT)
K= Ae(-Ea’/KBT)
activation energy
Ea = - gradient x R
Counting efficiency
counting efficiency = CPM / DPM
Partial pressure
PA = XA x P
Mole fraction
XA = number of moles of substance A/ total number of moles of all substances
Kp
Ka
relationship between pH and PKa
pH= 10 -PKa
PKa= -log10[pH]
Kw
Kw = [OH-][H+]
energy
E= hu
Beer Lambert Law
log10 (I0 / It) = OD= ecl
