Hello everyone,(adsbygoogle = window.adsbygoogle || []).push({});

I'm in my last year of A-level chemistry here in the UK, and am currently writing up my chemistry coursework. Its a project I was given on the kinetics of the reactions between magnesium ribbon and several different acids (I wanted to explore some much more exciting fields, but sadly couldn't!)

Anyway, I need some help on something...

i'm trying to use the 'arrhenius equation' to ascertain the activation energy/rate of reaction for a certain acid/particular molarity at a range of different temperatures, as an extension to the original project. I have the range of data (taken from 'inverted titrations' if you will!) for 5 different temperatures- aka the volume of gas produced every 10 seconds over a two minute period. (for example 8.8cm^2 after 10 seconds, 20.2cm^2 after 20 seconds)

my problem is I was visiting universities in the last lesson before the holidays started, and we were shown how to use k=Ae (-EA/ RT), and how this produces a graph of results... involving logarithms and... things. ahem. My maths isn't outstanding sadly, and I've hit a huge dead end with this. I also can't ask any staff as it's due in the day we return- about a weeks time.

So, heres my desparate plea. If anyone knows what I'm talking about and feels particulary kind, could you please either show me what to do, or point me in the right direction? If this is in the wrong forum or section of the site i apologise, I haven't been active here very long at all!

Thankyou in advance to any help

(p.s. does anyone know any websites that tell you the percentage error of simple scientific equipment such as burettes/ conical flasks/ measuring cylinders etc? or am i wishing on a star? heh)

<edited for a spelling mistake, theres probably more, its late!>

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# Arrhenius equations; A2 Chemistry coursework

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