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If Δ[ClO]/Δt​ at 298 K is 22.94×10–6 M/s, what is the rate of change in [Cl2]...

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)

Solutions

Expert Solution

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

queen_honey_blossom answered 2 years ago
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