Chlorine dioxide [ClO 2 ] oxidizes iodide ion in aqueous solution to elemental i
ID: 522928 • Letter: C
Question
Chlorine dioxide [ClO2] oxidizes iodide ion in aqueous solution to elemental iodine and is itself reduced to chlorite ion. Using the data below and graphical methods, determine whether the reaction follows zero, first or second order kinetics. Also, calculate the rate constant, k, for this reaction. Be sure to show ALL OF YOUR DATA PLOTS and how you made your determination. [10 points]
Time (seconds)
Chlorine dioxide Conc. in Moles Per Liter
0.00
4.77 x 10–4
1.00
4.31 x 10–4
2.00
3.91 x 10–4
3.00
3.53 x 10–4
5.00
2.89 x 10–4
10.00
1.76 x 10–4
30.00
2.40 x 10–5
50.00
3.20 x 10–6
Time (seconds)
Chlorine dioxide Conc. in Moles Per Liter
0.00
4.77 x 10–4
1.00
4.31 x 10–4
2.00
3.91 x 10–4
3.00
3.53 x 10–4
5.00
2.89 x 10–4
10.00
1.76 x 10–4
30.00
2.40 x 10–5
50.00
3.20 x 10–6
Explanation / Answer
Initial idea on data can be obtained from the plot of concentration of ClO2 vs time. The plot if is exponential sugests the reaction to be 1st order. This is the trend observed and is shown.
the reaction is 1st order, i.e -dCA/ dt= KCA, CA= concentration of ClO2
when integrated ln CA= lnCAO-Kt, where CA= concentration of ClO2 at any tiime and CAO= concentration of ClO2 at zero time.
the plot of lnCA vs time is shown below
from the plot the rate constant is slope = -K= -0.1, K=0.1/sec
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.