To determine the activation energy for the iodination of acetone, experimentally measure the rate constant at different temperatures and use the Arrhenius equation to plot ln(rate constant) against 1/T. The slope of this graph is -Ea/R, which allows calculation of the activation energy.
To determine the activation energy for the iodination of acetone, further experiments involving measurements of the reaction rate at different temperatures are required. By conducting these experiments, you can obtain the rate constant (k) at several temperatures. Once you have these values, you can utilize the Arrhenius equation to plot the natural logarithm (ln) of the rate constant against the inverse of the temperature in Kelvin degrees (1/T). The slope of this linear graph is equal to the negative activation energy divided by the universal gas constant (R). Specifically, the slope is -Ea/R, allowing you to calculate the activation energy (Ea) for the reaction. An alternative, more expedient approach is to derive the activation energy from the rate constant measurements at just two different temperatures using a two-point form of the Arrhenius equation. This method is beneficial when resources or time are limited.