Question

If Δ[ClO]/Δt​ at 298 K is 22.94×10–6 M/s, what is the rate of change in [Cl2] in the following reaction? 2ClO(g)= Cl2​(g)+O2​(g)

Answer 1

1) 2ClO(g) ---------------> Cl₂(g) + O₂(g)

Now, rate of reaction = -(1/2)*rate of disappearance of ClO = rate of formation of O₂ = rate of formation of Cl₂

or, rate of reaction = -(1/2)*d[ClO]/dt = d[Cl₂]/dt = d[O₂]/dt

Given d[ClO]dt = 22.93*10^-6 M/s

thus, d[Cl₂]/dt = d[O₂]/dt = (1/2)*d[ClO]/dt = 11.465*10^-6 M/s

2) ClO(g) + O₃(g) -----> O₂(g) + ClO₂(g)

Now, rate of reaction = -rate of disappearance of ClO = rate of disappearance of O₃ = rate of formation of O₂ = rate of formation of ClO₂

or, rate of reaction = -d[ClO]/dt = -d[O₃] = d[ClO₂]/dt = d[O₂]/dt

Given d[ClO]dt = 28.65*10^-3 M/s

Thus, d[O₃] = d[ClO₂]/dt = d[O₂]/dt = d[ClO]/dt =  28.65*10^-3 M/s