Question

Dinitrogen pentoxide (N2O5) decomposes as follows to nitrogen dioxide and nitrogen trioxide:
$$

N

2

​O

5

​(g)



NO

2

​(g)+NO

3

​(g)


Calculate the average rate of the reaction between consecutive measurement times in the following table.
Express every answer to two significant figures.
Rate 1 = molecules/(cm3·s)
Part 2 (1 point)

Rate 2 = molecules/(cm3·s)

Answer 1

Below are given the rates of the reaction.

Explanation:

Rate of a particular reaction is the concentration change of reactant or product divided by change in time. The rate of the reaction can be determined as below.

Given reaction:

N2O5 ------> NO2 + (g) + NO3 (g)

Rate = d [N2O5] / dt

Rate = - ([N2O5] final - [N2O5] initial) / t final - t initial

Rate 1 = - ([N2O5] final - [N2O5] initial) / t final - t initial

Rate 1 = - (1.855 x 10^12) - (1.905 x 10^12) / 1.85 - 0

Rate 1 =  2.7 x 10^10

Rate 2:  - ([N2O5] final - [N2O5] initial) / t final - t initial

Rate 2 = - (1.823 x 10^12) - (1.855 x 10^12) / 3.70 - 1.85

Rate 2 = 1.7 x 10^10

Rate 3:  - ([N2O5] final - [N2O5] initial) / t final - t initial