Answer to Question #145054 in General Chemistry for hunter

Question

3. The gaseous phase decomposition of dinitrogen pentoxide (N2O5) to nitrogen dioxide (NO2) and oxygen (O2) is given by,
2 N2O5(g) → 4 NO2(g) + O2(g)

For the reaction, the concentration of O2 was monitored and the following data were obtained.


Time/s: 0, 600, 1200, 1800, 3000, 4200
[O2] M: 0, 0.002, 0.004, 0.005, 0.006, 0.0072



a) What is the average rate of production of oxygen between 0 and 1200 seconds?


b) Is the rate of production of oxygen increasing or decreasing with time? Explain why this is so.

Answer 1

A) 2 N2O5(g) → 4 NO2(g) + O2(g)

0 +600+1200= 1800

1800/3 = 600seconds

B) yes it is increasing. As the decomposition of dinitrogen pentoxide (N2O5) to nitrogen dioxide (NO2) and oxygen (O2) increases