Question

The %Transmittance values were read from the spectrophotometer and the [A] values were calculated by changing %Transmittance to absorbance. Shown below is a plot of these data. [A] (M) 02030 do so by all 36 700 time (s) If this reaction had been a zero-order reaction, a plot of time v.s. [A] would have been linear. It is not. We will use the integrated rate laws to determine the order of the reaction, given these data. The rate laws are summarized on p.44 of the lab manual. To decide if the reaction is first order in A, plot time v.s. In[A]. Fill in the first three lines of the table, shown below. You need to calculate In[A] for the first three time points. time (s) % Transmittance [A] In [A] 0 15 30 45 60 97.32 98.57 99.02 1.18 x 10-2 6.25 x 10-3 4.26 x 10-3 3.23 x 10-3 2.60 x 10-3 99.26 3.23 x 10 -5.74 -5.95 75 99.40 Submit Answer Tries 0/99

Answer 1

The reaction is not first order as ln [A] versus time is not a straight line.

time (s) % Transmittance (A) In (A) 0 15 30 45 97.32 98.57 1.18 x 10-2 1-4.44 6.25 x 10-3 -5.08 4.26 x 10-3 -5.46 3.23 x 10-3 -5.74 2.60 x 10-3 -5.95 99.02 99.26 99.40 60 75

In [A] TTTTTT 20 60 40 Time, t(s)