ALL FORMULAE TO LEARN

Enthalpy equation (ΔH)

ΔH = -mcΔT/mols

m - mass

C- specific heat capacity

Ideal gas equation

pV = nRT

V - volume in $m^3$

R - ideal gas constant

T - in K

p - in Pa

Gibbs Free Energy Equation

ΔG = ΔH - TΔS

S - entropy in $kJ^{}K^{-1}mol^{-1}$

Entropy change of a reaction

ΔS° = ΣS°(products) - ΣS°(reactants)

ALL IN J K^-1mol^-1

^{(NOT kJ)}

Rate equation

Rate = K[A]^x[B]^y[C]^z

Where x y z are the order wrt A B C

Rate constant from half life

K = 0.693/t1/2

t1/2 measured in seconds

Only for FIRST ORDER reactions

Ka expression

Ka = [H+][A-] / [HA]

Kw expression (given numerical value)

Kw = [H+][OH-]

pH equation

pH = -log[H+]

[H+] = 10^-pH

E^ocell

E^ocell = E^ored - E^oox

in V

most positive E^o - least positive E^o

under standard conditions: 298K, 101kPa, 1M solutions

Charge in terms of current

Q = It

Q - in C

I - in Cs^-1

charge in terms of moles of electrons

Q = F x z

z - moles of e-

F - Faraday constant (charge per mole of e-)

Nernst Equation

E = E^o + (0.059/z)log[ox]/[red]

E = non-standard electrode potential, V

z - moles of e- transferred

feasibility formula (electrochem)

ΔG^o = -nFE^o_cell

reaction is feasibly if ΔG^o is NEGATIVE

n - moles of e- transferred

F - Faraday constant

G and Ecell in V

dilution equation

ViCi = VfCf

initial vol x initial conc = vol x conc after dilution

equation for number of carbon atoms from mass spectra

n = (100 x abundance of M+1 ion) / (1.1 x abundance of M⁺ ion)

pH directly from pKa (Henderson-Hasselbach equation)

pH = pKa + log([A^-]/[HA])