Question

A student runs an experiment in the lab and then uses the data to prepare an Arrhenius plot of the natural log of the rate constant (ln k) versus the inverse of the absolute temperature (1 / T). The general equation of the resulting line is given below. What is the activation energy for the reaction in kilojoules per mole? y = - 2.63 × 103 x + 27.3

Answer 1

Answer:

21.86582KJ

Explanation:

The graphical form of the Arrhenius equation is shown on the image attached. Remember that in the Arrhenius equation, we plot the rate constant against the inverse of temperature. The slope of this graph is the activation energy and its y intercept is the frequency factor.

Applying the equation if a straight line, y=mx +c, and comparing the given equation with the graphical form of the Arrhenius equation shown in the image attached, we obtain the activation energy of the reaction as shown.

Answer 2

Following are the solution to the given question:

Given:

Please find the given question.

To Find:

Ea=?

Solution:

$\to R=8.314 \ \frac{j}{\frac{mol}{k}}\\\\\to slope=-\frac{Ea}{R}=-2.63\times 10^3\\\\\to Ea=R\times slope$

         $=8.314\times 2.63\times 10^3\\\\=21865\ j\\\\=21.865\ kj$

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