The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by two step process shown below,
`O_(3)(g)+Cl(g) to O_(2)(g)+ClO(g)` … (i) [`K_(i)=5.2times10^(9) L*mol^(-1)*s^(-1)`
`ClO(g)+O_(2)(g) to O_(2)(g)+Cl(g)`…. (ii) [`K_(ii)=2.6times10^(10)l*mol^(-1)*s^(-1)`]
The closet rate constant for the overall reaction `O_(3)(g)+O(g) to 2O_(2)(g)` is:

Options

A. `1.4times10^(20)l*mol^(-1)*s^(-1)`
B. `3.1times10^(10)l*mol^(-1)*s^(-1)`
C. `5.2times10^(9)l*mol^(-1)*s^(-1)`
D. `2.6times10^(10)l*mol^(-1)*s^(-1)`

Answer

A

Explanation

On adding eq. (i) and and eq.(ii) wer get `O_(3)(g)+O(g) to 2O_(2)(g)`
Hence overall rate constant=`K_(i)K_(n)=5.2times10^(9)times2.6times10^(10)=1.4times10^(2)mol^(-1)Ls^(-1)`