Okay, so I’m completely stuck on this one chemistry problem about reaction rates. I’ve been staring at my notes for an hour, and I just can’t figure out how to apply the Arrhenius equation to this specific set of experimental data they gave us. It feels like I’m missing one key connection. Has anyone else hit a wall with this?
I feel you Arrhenius can be stubborn when data fights you If you have k values at several temperatures plot ln k against 1/T in Kelvin and look for a straight line The slope is minus Ea over R and the intercept is ln A If the plot curves something else might be going on
One angle to try is to make sure you are extracting k correctly If you used initial rates convert them to k with the rate law you think the reaction follows because k is the piece that goes into Arrhenius not the overall rate itself Also check units for R and for T in Kelvin tiny mistakes there wreck the slope
Sometimes the problem is that the data hides a mechanism change If the data hints at a break in the line that suggests a different active pathway at high temperature Arrhenius still applies to each regime but you might need two lines and two Ea values
I get the sense you are chasing a single clean trick but Arrhenius isnt magical if your data is noisy Consider doing a rough fit and then see if Ea is reasonable compared to literature It is not a moral failing if it does not line up perfectly
Could it be you are mixing up units for temperature or using C instead of K That little error will shift the whole line and make you think you are missing something key
Maybe the problem is not about math but about framing Arrhenius is a relation between temperature and rate constants If the data is all at the same temperature or if they gave you a pseudo first order setup the connection might be different than you expect