Arrhenius Equation

Introduced to in CHE102

Arrhenius Equation: $k=A{e}^{\frac{-E_a}{RT}}$

• k = rate constant
• A = pre-exponential factor
• $E_a$ = Activation Energy (in the same units as R * T)
• R = Universal Gas Constant
• T = Absolute Temperature (in Kelvin)

Simplified Logarithmic Form §

$ln(k)=-\frac{E_a}{RT}+ln(A)$

Increasing temperature increases K, reactions proceed faster at higher temperatures

Increasing the Activation Energy $E_a$ decreases K, makes the reaction slower

$ln(\frac{k_1}{k_2})=\frac{E_a}{R}(\frac{1}{T_2}-\frac{1}{T_1})$