Ask Question
17 May, 14:18

The rate constant of a reaction is 4.7*10-3 s-1 at 25°C, and the activation energy is 33.6 kJ/mol. What is k at 75°C?

+1
Answers (1)
  1. 17 May, 18:16
    0
    k is 3,18*10⁻² s⁻¹ at 75°C

    Explanation:

    following Arrhenius equation:

    k = k₀*e^ (-Ea/RT)

    where k = rate constant, k₀ = frequency factor, Ea = activation energy, R = universal gas constant T=absolute temperature

    then for T₁=25°C = 298 K

    k₁ = k₀*e^ (-Ea/RT₁)

    and for T₁=75°C = 348 K

    k₂ = k₀*e^ (-Ea/RT₂)

    dividing both equations

    k₂/k₁ = e^ (-Ea/RT₂+Ea/RT₁)

    k₂ = k₁*e^[-Ea/R * (1/T₂-1/T₁) ]

    replacing values

    k₂ = k₁*e^[-Ea/R * (1/T₂-1/T₁) ] = 4,7*10⁻³ s⁻¹ * e^[-33.6*1000 J/mol / 8.314 J/molK * (1 / 348 K - 1/298 K) ] = 3,18*10⁻² s⁻¹

    thus k is 3,18*10⁻² s⁻¹ at 75°C
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “The rate constant of a reaction is 4.7*10-3 s-1 at 25°C, and the activation energy is 33.6 kJ/mol. What is k at 75°C? ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers