posted by Martin on .
Calculate the rate at which N2O4 is formed in the following reaction at the moment in time when NO2 is being consumed at a rate of 0.0521 M/s.
2NO2(g) <-> N2O4 (g)
I am not really sure how to go about this problem.
rate = k (N2O4)
d(NO2)/dt = -2 d(N2O4)/dt
This is what I have so far
Isn't the rate of appearance of N2O4 just 1/2 that of disappearance of NO2?