The correct option is D Rate of disappearance of N2O5 is twice the O2 production rate
2N2O5→4NO2+O2
rate=12(−d[N2O5]dt)=14(d[NO2]dt)=d[O2]dt
a) d[NO2]dt=4d[O2]dt
Thus NO2 production rate is four times the O2 production rate.
b) We know,
12(−d[N2O5]dt)=d[O2]dt
So O2 production rate is half the rate of disappearance of N2O5.
c)12(−d[N2O5]dt)=14(d[NO2]dt
(−d[N2O5]dt)=12(d[NO2]dt)
So, Rate of disappearance of N2O5 is one-half of NO2 production rate.
d) 12(−d[N2O5]dt)=d[O2]dt
⇒(−d[N2O5]dt)=2d[O2]dt
So, rate of disappearance of N2O5 is twice the O2 production rate.