In the picture above, real experimental data is presented for the decomposition

Question

In the picture above, real experimental data is presented for the decomposition reaction wherein N2O5 decomposed to NO2 and O2 at 30 degrees C. Use the data provided to answer the following 3 questions:

a) Assume that the order of the reaction with respect to N2O5 is either 1st or 2nd. What is the order? Support your reasoning.

b) Give the rate constant for the reaction with proper units.

c) Calculate t1/2 for this reaction.

2 5 1.40 1.30 1.201 1.10 1.00 0.90 0.80 0.70 0.60 0.50 0,40 0.30 0.20 Average rate for 15 min period 15 min to decrease [N205] from 1.22 to 1.10 Rate of reaction0.12 molVt mol L min = 0.0080 15 min Instantaneous rate when [N205] = 0.34 M AIN 00.22 mol/L-0.42 molVL (6.3 h-4.0 h) (60 min/h) Instantaneous rate At mol L min 0.0014 2 Average rate for 6.5 to 9.0h 0.42 mol .min Rate of reaction = 0.00080 [N205] At 1.0 2.0 3.0 4.0 5.0 6.0 7.0 8.09.0 10 11 Time (t), hours Brooks Cole, Cengage Leaming

Explanation / Answer

a) The time taken to reduce the concentration of [N2O5] from 1.4 mol/L to 0.7 mol/L and 0.7 mol/L to 0.35 mol/L is same. The constant half life suggests the reaction is first order in kinetics with respect to [N2O5] concentration.

b) rate constant = 6.67 x 10^-3 min-1

c) t1/2 = 0.693/k = 0.693/6.67 x 10^-3 = 103.9 min

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