Ask Question
17 June, 00:31

The rate constant of a reaction is 5.8 * 10-3 s-1 at 25°c, and the activation energy is 33.6 kj/mol. what is k at 75°c? enter your answer in scientific notation.

+3
Answers (1)
  1. 17 June, 00:43
    0
    k₂ = 4.06 x 10⁻² s⁻¹.

    Explanation:

    From Arrhenius law: K = Ae (-Ea/RT)

    where, K is the rate constant of the reaction.

    A is the Arrhenius factor.

    Ea is the activation energy.

    R is the general gas constant.

    T is the temperature.

    At different temperatures:

    ln (k₂/k₁) = Ea/R [ (T₂-T₁) / (T₁T₂) ]

    k₁ = 5.8 * 10⁻³ s⁻¹, k₂ = ?, Ea = 33600 J/mol, R = 8.314 J/mol. K, T₁ = 298.0 K, T₂ = 348.0 K.

    ln (k₂/5.8 * 10⁻³ s⁻¹) = (33600 J/mol / 8.314 J/mol. K) [ (348.0 K - 298.0 K) / (298.0 K x 348.0 K) ] = (4041.37) (4.82 x 10⁻⁴) = 1.9479. Taking exponential of both sides:

    (k₂/5.8 * 10⁻³ s⁻¹) = 7.014.

    ∴ k₂ = 4.06 x 10⁻² s⁻¹.
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “The rate constant of a reaction is 5.8 * 10-3 s-1 at 25°c, and the activation energy is 33.6 kj/mol. what is k at 75°c? enter your answer ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers