`N_(2)O_(5)` decomposes to `NO_(2)` and`O_(2)` and follows first order kinetics. After `50` minutes the pressure inside the vessel increases from 50 mm Hg to `87.5 mmHg`. The pressure of the gaseous mixture afte 100 minute at constant temperature will be :

The reaction 2N_(2)O_(5)(g)rarr4NO_(2)(g)+O_(2)(g) follows first order kinetics. The pressure of a vessel containing only N_(2)O_(5) was found to increase from 50 mm Hg to 87.5 mm Hg in 30 mim. The pressure exerted by the gases after 60 min. will be (Assume temperature remains constant):

The reaction 2N_(2)O_(5)(g)rarr4NO_(2)(g)+O_(2)(g) follows first order kinetics. The pressure of a vessel containing only N_(2)O_(5) was found to increase from 50 mm Hg to 87.5 mm Hg in 30 mim. The pressure exerted by the gases after 60 min. will be (Assume temperature remains constant):

The decomposition of gaseous Cl_(2)O_(7) to gaseous Cl_(2) and O_(2) at 400K is a first order reaction . After 55 s , the pressure of Cl_(2)O_(7) falls from 0.062 to 0.044 atm . Calculate the pressure of Cl_(2)O_(7) after 100s.

N_(2)O_(5(g)) is at a pressure of 0.5 atm. After 100 s the pressure of the decomposition mixture is 0.512 atm. Calculate the rate constant.