The reaction ,
`2N_(2)O_(5)rarr4NO_(2)+O_(2)`
was studdied and the following data were collected :

Determine (i) order the reaction (ii) the rate law and (iii) rate constant for the reaction

Explanation

Let the rate law for the reaction be
Rate =`k[N_(2)O_(5)]^(x)`
`34xx10^(-5)=k[1.13xx10^(-2)]^(x)`
`25xx10^(-5)=k[0.84xx10^(-2)]^(x)`
`(25xx10^(-5))/(25xx10^(-5))=([1.13xx10^(-2)]^(2))/[0.84xx10^(-2)]^(x)`
`1.36=[1.345]^(x)`
Order of the reaction is 1. Rate law = `k[N_(2)O_(5)]`
`k=("Rate")/([N_(2)O_(5)])=(34.xx10^(-5))/(1.13xx10^(-2))=30.08xx10^(-3) "min"^(-1)`