I investigated the Arrhenius equation using the reaction between potassium iodate (containing the IO3- iodate ion) and sodium bisulfite (containing the HSO3- hydrogen sulfite ion. The ionic equations for the reaction’s two stages are as follows:
IO3- (aq) + 3HSO3- (aq) -----> I- (aq) + 3SO42- (aq) + 3H+ (aq)
5 I- (aq) + 6H+ (aq) + IO3- (aq) -----> 3I2 (aq) + 3H2O (l)
I rearranged the Arrhenius equation to give: ln(k)=(-Ea)/R)(1/T) + ln(A)
I changed the temperature of the reaction and timed the speed of the reaction, which I used to calculate the values of k. I then graphed the relation between ln(k) and 1/T , with the slope giving –Ea/R.
My graph ended up having a slope of -0.0003, so I obtained an activation energy of 0.00024942 J/mol.
I was wondering if anyone had a theoretical value of the activation energy of this reaction I can compare my experimental value to?