Chemical Kinetics

For a reaction, aA + bB -> cC + dD

Average rate = -$1/a {Δ[A]}/{Δt}$ = – $1/b {Δ[B]}/{Δt}$ = – $1/c {Δ[C]}/{Δt}$ = -${Δ[D]}/{Δt}$

Rate law: Rate = $k [A]^a * [B]^b$

k = ${2.303}/t log_{10} {[A]_o}/{[A]_t}$ (For first order reaction)

$t_{1/2} = {0.693}/k$ (For first order reaction)

$k = {[A]_o – [A]_t}/{t}$ (For zero order reaction)

$t_{1/2} = {[A]_o}/{2k}$ (For zero order reaction)

$k = A e^{-{Ea}/{RT}}$ (Arrhenius equation)

$log_{10}k = log_{10}A – {E_a}/{2.303 RT}$

$log_{10} {k_2}/{k_1} = {E_a (T_2 – T_1)}/{2.303 R T_1 T_2}$