Using ln(k₂/k₁) = (Eₐ/R)[(T₂-T₁)/(T₁T₂)]; ln(k₂/k₁) = (60000/8.314)[(300)/(600×300)] ≈ 6.2; k₂/k₁ ≈ 500
For second-order: t₁/₂ = 1/(k[A]₀); 100 = 1/(k × 0.5); k = 0.04 M⁻¹s⁻¹
Adding all steps and canceling intermediates (Cl, H): Cl₂ + H₂ → 2HCl
1/[A] = 2 + 0.4(5) = 2 + 2 = 4; [A] = 1/4 = 0.25 M
Catalyst lowers Eₐ (forward and reverse) without changing ΔH, reaction enthalpy change
For elementary reactions, rate law exponents = stoichiometric coefficients. Rate = k[A]²[B]
k = A·exp(-Eₐ/RT) = 2 × 10¹³ × exp(-50000/8.314×300) = 2 × 10¹³ × exp(-20.03) ≈ 3.4 × 10⁻³ s⁻¹
Rate constant k is independent of reactant concentration; it depends on T, nature of reactants, and catalyst
If doubling concentration increases rate by 4 times (2²), reaction is second order
For first-order: k = 0.693/t₁/₂ = 0.693/30 = 0.0231 min⁻¹ ≈ 0.023 min⁻¹