Question

The rate of decomposition of N2O5 in CCl4 at 317 K has been studied by monitoring the concentration of N2O5 in the solution. 2 N2O5(g) → 4 NO2(g) + O2(g) Initially the concentration of N2O5 is 2.36 M. At 177 minutes, the concentration of N2O5 is reduced to 2.16 M. Calculate the average rate of this reaction in M/min.

Answer 1

Average rate of reaction is 0.000565 M/min

Step-by-step explanation:

Applying law of mass action for the given reaction:

Average rate =
`-(1)/(2)([N_(2)O_(5)])/(\Delta t)=(1)/(4)(\Delta [NO_(2)])/(\Delta t)=(\Delta [O_(2)])/(\Delta t)`

Where,
`-(1)/(2)([N_(2)O_(5)])/(\Delta t)` represents average rate of disappearance of
`N_(2)O_(5)`,
`(1)/(4)([NO_(2)])/(\Delta t)` represents average rate of appearance of
`NO_(2)` and
`([O_(2)])/(\Delta t)` represents average rate of appearance of
`O_(2)`

Here,
`-([N_(2)O_(5)])/(\Delta t)` =
`-((2.16-2.36))/((177-0))M/min=0.00113M/min`

So average rate of reaction =
`[tex]-(1)/(2)([N_(2)O_(5)])/(\Delta t)`[/tex] =
`(1)/(2)* (0.00113M/min)=0.000565M/min`