Answer to Question #6498 in Inorganic Chemistry for Danielle

Question

Consider the reaction: 4 NO2(g) + O2(g) ----> 2N2O5(g)
At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of .0013 M/s.
a) At what rate is molecular oxygen being consumed?
b) At what rate is dinitrogen pentoxide being produced?

Answer 1

4NO2(g) + O2(g) ---->2N2O5(g)
In the case when nitrogen
dioxide
is being consumed at the rate of 0.0013 M/s,
oxygen being consumed with the
rate of 1/4 * 0.0013= 0.000325 and dinitrogen pentoxide being produced with the
rate 2/4 *0.0013=0.00065 M/s.