Under certain conditions, the average rate of appearance of oxygen gas in the reaction: 2O3(g)–>3O2(g)?

is 1.2 x 10^-3 atm s-1. What’s the common fee for disappearance of O3?

Utilizing the balanced coefficients within the equations we all know tips on how to relate the speed, d/dt, of product to a reagent;

(1/3)d(O2)/dt = 1/2(d(O3)/dt)

subsequently,

d(O3)/dt = (2/3)d(O2)/dt = (2/3)(1.2×10^-3 atm/s) = 8.0×10^-4 atm/s