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Zero-order reaction is when the rate of a reaction is independent of the
concentration of a reactant: rate=k [A]0 = k. Graph of [A] vs time is a straight line, with
a negative slope = rate. [A]t = [A]0 – kt.
First-order reaction is where the rate doubles when concentration doubles: rate =k
[A]1. Graph of [A] against time is an exponential curve; graph of ln [A] vs. t is a
straight line with a negative slope where slope = k the rate constant. Half-life of a first
order reaction is a constant; t1/2=0.693/k. Integrated form of first order equation: ln
ln [A]t = − kt + ln [A]0 OR ln [A]0 – ln[A]t = kt OR o [ A]0
; [A]t = [A]0e-kt (the last two equations are given in the Data Book). o
irst-order reaction is where the rate doubles when concentration doubles: rate =k
[A]1. Graph of [A] against time is an...
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- Spring '10