Answer:
[O₃]= 8.84x10⁻⁷M
Explanation:
The photodissociation of ozone by UV light is given by:
O₃ + hν → O₂ + O (1)
The first-order reaction of the equation (1) is:
[tex] rate = k [O_{3}] = - k \frac{\Delta [O_{3}]}{\Delta t} [/tex] (2)
where k: is the rate constant and Δ[O₃]/Δt: is the variation in the ozone concentration with time, and the negative sign is by the decrease in the reactant concentration
We can get the following expression of the first-order integrated law of the reaction (1), by resolving the equation (2):
[tex] [O_{3}]_{t} = [O_{3}]_{0} \cdot e^{-kt} [/tex] (3)
where [O₃](t): is the ozone concentration in the elapsed time and [O₃]₀: is the initial ozone concentration
We can calculate the initial ozone concentration using equation (3):
[tex] [O_{3}]_{t} = 5.0 \cdot 10^{-3}M \cdot e^{-(1.0\cdot 10^{-5}s^{-1}) (\frac{10d \cdot 24h \cdot 3600 s}{1d \cdot 1h})} = 8.84 \cdot 10^{-7}M [/tex]
So, the ozone concentration after 10 days is 8.84x10⁻⁷M.
I hope it helps you!
