The decomposition of azo methane, at certain temperature according to the equation
`(CH_(3))_(3)N_(2)rarr C_(2)H_(5)+N_(2)` is a first order reaction.
After 40 minutes from the start, the total pressure developed is found to be `350 mm Hg` in place of initial pressure `200 mm Hg` of axo methane . The value of rate constant `k` is `-`

The decomposition of azo methane, at certain temperature acccording to the equation (CH_(3))_(2)N_(2)toC_(2)H_(6)+N_(2) is a first order reaction. After 40 minutes from the start, the total pressure developed is found to be 350 mm Hg in place of initial pressure 200 mm Hg of azo methane. The value of rate constant k is :

The decomposition of azo methane, at certain temperature acccording to the equation (CH_(3))_(2)N_(2)toC_(2)H_(6)+N_(2) is a first order reaction. After 40 minutes from the start, the total pressure developed is found to be 350 mm Hg in place of initial pressure 200 mm Hg of azo methane. The value of rate constant k is :

The decomposition of azo methane, at certain temperature acccording to the equation (CH_(3))_(2)N_(2)toC_(2)H_(6)+N_(2) is a first order reaction. After 40 minutes from the start, the total pressure developed is found to be 350 mm Hg in place of initial pressure 200 mm Hg of azo methane. The value of rate constant k is :

The decomposition of N_(2)O_(5) according to the equation, 2N_(2)O_(5) (g) rarr 4NO_(2) (g) + O_(2) (g) is a first order reaction, After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm Hg and on completion, the total pressure is 584.5 mm Hg. Calculate the rate constant of the reaction.

The decompasition N_(2)O_(5) acccording to the equation. N_(2)O_(5)rarr4NO_(2)(g)+O_(2)(g) is a first order reaction. After 30 minutes from the start of the decomposition is a closed vessel, the total pressure developed is found to be 284. 5 mm Hg and on completion the total pressure is 284.5mm Hg. Calculate the rate constant of the reaction