00:01
In this question, we have to determine what is the activation energy of some reaction that at 10 degrees celsius happens 1 .878 times faster than it happens at 5 degrees celsius.
00:14
So in this question, we have to use this expression, actually this relation between the reaction rate and this exponential.
00:22
So the reaction rate is proportional to this exponential.
00:25
So we begin by dividing this reaction rate by this reaction rate.
00:31
So the left -hand side we get e to minus the activation energy divided by k times the temperature which is 10 degrees celsius but we have to convert it to kelvin before plugging this equation and that conversion is very simple.
00:49
You just have to add 273 to the celsius temperature.
00:54
So this is 200 and and this is divided by the exponential of minus the activation energy divided by k times 5 degrees celsius, which is 278 kelvin's.
01:12
And this is equal to 1 .878 times x divided by x.
01:17
As you can see on the right hand side, we have x both on the numerator and the denominator, so we can simplify it.
01:23
And we are left with 1 .878.
01:29
Now, we have to work on the left -hand side of this equation...