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I am having serious problem at plotting the graph for the reaction between Bromide ion and Bromate(V) ion in Acid Solution. The Arrhenius euqation is:

[tex]k= Ae^{-E_a/RT}[/tex] Taking logarithms on both sides, the equation becomes: [tex]ln k = ln A + E_a/R (1/T) [/tex]

So generally, a graph of ln k versus 1/T is plotted. However, I don't need to find k in my experiment, so it is suggested that a graph of ln (1/t) versus 1/T is plotted, where t is the time required for the complete disappearing of the red colour.

of course, if two rate constant values are compared, like: [tex]ln (k1/k2) = -E_a/R (1/T1 - 1/T2) [/tex], the ln(ka/k2) can be replaced by ln(rate1/rate2), since rate is proporational to k....

Can anybody kindly enough to explain to me why a ln (1/t) versus 1/T is plotted? *confusing*

Thanks!!

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# To determine the activation energy

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