Concentrations measured as a function of time when gaseous `N_(2)O_(5)` at initial concentration of `0.0200 M` decomposes ot gaseous `NO_(2)"and"O_(2) "at" 50^(@)C.`The change in concentration with time is given by the following graph.

The instantaneous rate of disappearance of `N_(2)O_(5)` at the beginning of the reaction is :

Concentrations measured as a function of time when gaseous N_(2)O_(5) at initial concentration of 0.0200 M decomposes ot gaseous NO_(2)"and"O_(2) "at" 50^(@)C. The change in concentration with time is given by the following graph. The rate of decomposition of N_(2)O_(5) during the period 300-400 s is :

Concentrations measured as a function of time when gaseous N_(2)O_(5) at initial concentration of 0.0200 M decomposes ot gaseous NO_(2)"and"O_(2) "at" 50^(@)C. The change in concentration with time is given by the following graph. The rate of formation of O_(2) during the period 600-700 s is :

Findingf concentration and time : The rate constant for the decomposition of gasous N_(2)O_(5) at 55^(@)C is 1.7xx10^(-3)s^(-1) . If the initial concentration of N_(2)O_(5) after five half-lives ? How long will it take for the N_(2)O_(5) concentration to fall to 12.5% of its initial values ? Strategy : Because the unit of rate constant is time^(-1) , the decomposition of N_(2)O_(5) is a first order reaqction. To find [N_(2)O_(5)] after n half lives, multiply its initial concentration by (1//2)^(n) since [N_(2)O_(5)] drops by a factor of 2 during each successive haslf-life.

2N_(2)O_(5)rarr4NO_(2)(g)+O_(2)(g) , The above reaction is completed in a closed vessel . It is observed that the concentration of NO_(2) is increased by 4xx10^(-2)"mol.L"^(-1) in 5 second . Calculate the rate of disappearance of N_(2)O_(5)

The thermal decomposition of N_(2)O_(5) occues as: 2N_(2)O_(5) rarr 4NO_(2)+O_(2) Experimental studies suggest that rate of decomposition of N_(2)O_(5) rate of formation of NO_(2) or rate of formation of O_(2) all becomes double if concentration of N_(2)O_(5) is doubled. If rate of formation of O_(2) is 16 g//hr then rate of decomposition of N_(2)O_(5) and rate of formation of NO_(2) respectively is

The reaction, 2N_(2)O_(5)rarr 4NO_(2)+O_(2) , shows an increase in concentration of NO_(2) by 20xx10^(-3) mol litre^(-1) in 5 second. Calculate: (a) rate of appearance of NO_(2) , (b) rate of reaction and (c ) rate dissappearance of N_(2)O_(5) .

The rate constant of the decomposition of N_(2)O_(5) is 6.0 X10^(-4) s^(-1) .At what time will the initial concentration of 1M be reduced to 0.2 M is the reaction of the first order ?

The decompoistion of N_(2)O_(5) in C CI_(4) solution at 318 K has been studied by monitoring the concentration of N_(2)O_(5) in the solution. Initially, the concentration of N_(2)O_(5) is 2.33 M and after 184 min , it is reduced to 2.08 M . The reaction takes place according to the equation: 2N_(2)O_(5) rarr 4NO_(2) + O_(2) Calculate the average rate of this reaction in terms of hours, minutes, and seconds. What is the rate of Production of NO_(2) during this period?