The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below:
`O_(3)(g)+Cl^(.)rarrO_(2)(g)+ClO^(.)(g)…(i)`
`k_(i)=5.2xx10^(9)" L mol"^(-1)s^(-1)`
`ClO^(.)(g)+O^(.)(g)rarrO_(2)(g)+Cl^(.)(g).......(ii)`
`k_(ii)=2.6xx10^(10)"L mol"^(-1)s^(-1)`
The closest rate constant for the overall reaction
`O_(3)(g)+O^(.)(g)rarr2O_(2)(g)` is :

Options

A. `1.4 xx 10^(20) L mol^(-1) s^(-1)`
B. `3.1 xx 10^(10) L mol^(-1) s^(-1)`
C. `5.2 xx 10^(9) L mol^(-1) s^(-1)`
D. `2.6 xx 10^(10) L mol^(-1) s^(-1)`

Answer

A

Explanation

On adding eq. (i) and eq. (ii) we get
`O_(3)(g) + O(g) to 2O_(2)(g)`
Hence overall rate constant `=K_(i) xx K_(ii)`
`=5.2 xx 10^(9) xx 2.6 xx 10^(10) ~~ 1.4 xx 10^(20) mol^(-1) Ls^(-1)`