**Question 1:**

The rate constant k of a chemical reaction increases with the absolute temperature T. This increase follows the equation below which is called the Arrhenius equation.

** k = Ae ^{-(Ea/RT)}**

Where E_{a} is the activation energy for the reaction, R is the gas constant and A is called the pre-exponential factor which is a constant for a given reaction. Sketch the shape of the graph of k versus T labelling the axes.

**Question 2: The Arrhenius Equation **

**k = Ae ^{-(Ea/RT) }**

Write the Arrhenius equation in the form of natural-logs.

**Solution 1:**

From the Arrhenius equation one can plot k against T as in below Figure.

**sketch of k against Tfor the Arrhenius equation. **

In above Figure it is difficult to read as at high temperatures a small change in T gives drastic changes in the rate constant k but at low temperatures a large change in T gives a negligible change in k. It would be much better if we can rearrange the Arrhenius equation to enable us to have a linear (straight line) graph.

**Solution 2:**

We can go from the exponential form of the Arrhenius equation to the natural-log form by:

(1) taking natural logs on both sides,

(2) the log on the right is a product of two terms which can be separated as the sum of two logs,

(3) the second term on the right is a natural-log of an exponential which is just equal to the exponent.

**ln (k) = ln [Ae ^{-(Ea/RT)}] **

**ln (k) = ln [A] + ln [e ^{-(Ea/RT)}] **

**ln (k) = [ln (A) – E _{a}/RT]**