Hey guys, im new to this place but I thought id post this up....

As part of a simulated practical I need to use the Arrhenius equation to find the activation energy of this reaction in different temperatures.

Now the data I collected is the volume versus the time taken up to 20 mins, for each temperature, I did 5 temps as a friend of mine did 5 more.

Now I know that the Arrhenius Equation can be Natural Log and will look like this:

ln(k) = -E/R x 1/T + ln(A)

But im stuck after I plotted the graph of different temps.

I know that the reaction is first order however I have no idea what to do, I think i might be able to draw a graph of 1/T against ln(k) however I dont have ln(k) or k for that matter.