The rule of thumb that the rate of reaction doubles for a 10 degrees C increase in temperature...


The rule of thumb that the rate of reaction doubles for a 10° C increase in temperature occurs only at a specific temperature for a given activation energy. Develop a relationship between the temperature and activation energy for which the rule holds. Ignore any variation of concentration with temperature.

Logarithmic Form of the Arrhenius Law:

The Arrhenius Law states that the rate constant of a reaction is related to the frequency factor, activation energy, and temperature, where R is the universal gas constant (8.314 J / mol K).

{eq}\displaystyle \ln \dfrac{k_2}{k_1} = \dfrac{-E_{\text{a}}}{R} \left( \dfrac{1}{T_2} - \dfrac{1}{T_1} \right) \\ {/eq}

The equation above is the logarithmic form of the Arrhenius Law.

Answer and Explanation: 1

Become a member to unlock this answer!

View this answer

Let the temperature be T. The rate constant ratio is 2 to account for the rate doubling. Isolating the activation energy, we get:

{eq}\ln 2 =...

See full answer below.

Learn more about this topic:

Arrhenius Acid: Definition & Examples


Chapter 16 / Lesson 2

What is an Arrhenius acid? Learn the definition of Arrhenius acid and the aqueous acid equation according to the theory, then see Arrhenius acid examples.

Related to this Question

Explore our homework questions and answers library