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?
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.