Here we will determine the activation energy for a reaction using k values determined at different temperatures. We begin by taking the reciprocal of the temperature in Kelvin. So we must first convert the temperature to Kelvin, then reciprocate those values. Then take the natural log of the k values. Once we've done that, then we could plot the data and determine the slope of the line. The plot is a straight line. The equation gives us the slope value, negative 5,638. According to the Uranus equation, the slope is equal to the negative activation energy divided by the ideal gas law constant. In this case, we'll set negative 5,638 equal to negative EA over R. The double negatives cancel and solving for the activation energy and converting it to kilojoules. We end up with 46.9 kilojoules. We could also determine the activation energy by substituting values of temperature and rate constants into the Uranus equation. Solving for the activation energy, the rearranged Uranus equation looks like this. Now we could pick any pair of temperature and rate constant values and substitute them into the equation. I picked the first two and came up with 47.2 kilojoules. We could also pick other pairs and determine that the activation energy is very close to 47.2. I prepared a spreadsheet to show this. Ficking the possible combinations or pairs of temperature and rate constants. I come up with six slightly different activation energies. But the average of the V6 is 46.9 kilojoules with a standard deviation of only 0.8.