The value of `K_(c )` for the reaction `3O_(2)(g) hArr 2O_(3)(g)` is `2.0xx10^(-50)` at `25^(@)C`. If the equilibrium concentration of `O_(2)` in air at `25^(@)C` is `1.6xx10^(-2)`, what is the concentration of `O_(3)`?

Explanation

`3O_(2)(g) hArr 2O_(3)(g)`
`K_(c) =[[O_(3)]^(2)]/[[O_(2)]^(3)] " or " (2.0 xx 10^(-50)) =[[O_(3)]^(2)]/((1.6 xx 10^(-2))^(3))`
`" or " " " [O_(3)]^(2) =(2.0 xx 10^(-50)) xx(1.6 xx 10^(-2))^(3)`
`[O_(3)]^(2) =8.192 xx 10^(-56) " or " [O_(3)] =(8.192 xx 10^(-56))^(1//2) =2.86 xx 10^(-28)M.`