Question

The following data were collected for dimerization of ClO to Cl2O2 at 298 K.
0 seconds 2.60×10^11
1 seconds 1.08×10^11
2 seconds 6.83×10^10
3 seconds 4.99×10^10
4 seconds 3.93×10^10
5 seconds 3.24×10^10
6 seconds 2.76×10^10
Plot [ClO] and [Cl2O2] as a function of time and determine the instantaneous rates of change in both at 1s. Please explain how everything is determined.

6. The following data were collected for the dimerization of CIO to CI:O2 at 298 K. (13.39) Time (s) [CO] O 2.60 10" 1.08 x 10" 2 6.83 x 100 3 4 .99 x 100 3.93 x 10 5 3.24 x 100 6 2.76 x 100 Plot (CIO) and (CI:O) as a function of time and determine the instantaneous rates of change in both at Is.

Answer 1

The reaction is second order as shown below: For a second order reaction: 1/[CO] = 1/[CLO]o + kt where [CO] is the concentration at time t, [CLOJo is initial concentration and k is rate constant From the data: A graph of 1/[CLO] vs time gives a straight line => reaction is second order Time(s) CIO 1/[CO] 0 2.60E+11 3.85E-12 1.08E+119.26E-12 2 6.83E+10 1.46E-11 3 4.99E+102.00E-11 4 3.93E+102.54E-11 3.24E+10 3.09E-11 6 12.76E+10 3.62E-11 5 4E-111 3.5E-11 3E-11 2.5E-11- 1[CIO] 2E-11 1.5E-11- 5E-12 0 1 2 3 4 5 6 Time (s)

Rate change of ClO concentration for period of 1 s to 2 s = [(1.08 x 10¹¹) -(6.83 x 10¹⁰)]
= 3.97 x 10¹⁰ molecules /sec.cm³

Rate change of ClO concentration for period of 4 s to 5 s = [(3.93 x 10¹⁰) -(3.24 x 10¹⁰)]
= 0.69 x 10¹⁰ molecules /sec.cm³

Second is smaller then first because order of reaction is 2.