k = A * e^(-Ea/RT). A = pre-exponential (frequency) factor — represents collision frequency with correct orientation. Ea = activation energy (J/mol or kJ/mol). R = 8.314 $\frac{J}{mol.K}$. Logarithmic form: ln(k) = ln(A) - $\frac{Ea}{RT}$. Plot ln(k) vs 1/T: straight line, slope = -Ea/R, intercept = ln(A). Two-temperature form: ln$\frac{k2}{k1}$ = $\frac{Ea}{R}$(1/T1 - 1/T2). Using log: log$\frac{k2}{k1}$ = $\frac{Ea}{2.303R}$(1/T1 - 1/T2). Temperature coefficient: for most reactions near room temperature, rate doubles for every 10 K rise (k2/k1 ≈ 2 for T2 - T1 = 10). A higher Ea means stronger temperature dependence. At T -> infinity, k -> A (maximum possible rate constant).