Question

The decomposition of N2O5 can be described by the equation

2N2O5(soln)⟶4NO2(soln)+O2(g)

Given the data in the table for the reaction at 45 °C in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval.

t (s)	[N2O5] (M)
0	2.463
165	2.220
506	1.792
815	1.475

interval: 0 s to 165 s average rate of reaction: M/s

interval: 165 s to 506 s average rate of reaction: M/s

interval: 506 s to 815 s average rate of reaction: M/s

Nitrogen pentoxide decomposes to produce nitrogen dioxide and oxygen according to the equation.

2N2O5(g)⟶4NO2(g)+O2(g)2N2O5(g)⟶4NO2(g)+O2(g)

The following data were collected for this reaction at 298K. Calculate the rate of change for N₂O₅ between 100100 s and 300300 s.

Time (s)	[N2O5] (M)	[NO2] (M)	[O2] (M)
0	0.0200	0	0
100	0.0169	0.0063	0.0016
200	0.0142	0.0115	0.0029
300	0.0120	0.0160	0.0040
500	0.0086	0.0229	0.0057
700	0.0061	0.0278	0.0070

M/s

Answer 1

Answer:

I. The rate can be written as;

Rate of disappearance of N₂O₅, r_d = d[N₂O₅]/dt

Rate of reaction = -1/2 x r_d

For 0 - 165 s

rate_avg = - 1/2 x (2.220 - 2.463)/(165 - 0) = 7.36 x 10^-4 M/s

For 165 - 506 s

rate_avg = - 1/2 x (1.792 - 2.220)/(506 - 165 ) = 6.27 x 10^-4 M/s

For 506 - 815 s

rate_avg = - 1/2 x (1.475 - 1.792)/(815 - 506) = 5.12 x 10^-4 M/s

II. Similar to the above question, the rate of change of N₂O₅ can be given by the simple relation;

r_d = d[N₂O₅]/dt = (0.0120 - 0.0169)/(300-100) = -2.45 x 10^-5 M/s

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