For the reaction; 2N2O5g→4NO2g+O2gif the concentration of NO2 increases by 5.2×10-3M 100 seconds then the rate of the reaction is

$2 N_{2} O_{5 (g)} \to 4 {NO}_{2 (g)} + O_{2 (g)}$

Rate of appearance of ${NO}_{2}$ is $\frac{change in the concentration of {NO}_{2}}{time}$ $= \frac{5.2 \times 10^{- 3}}{100}$

$5.2 \times 10^{- 5} M . s^{- 1}$

rate of reaction $= \frac{1}{4} \frac{d [{NO}_{2}]}{dt}$

$= \frac{1}{4} \times 2.5 \times 10^{- 5}$

$= \frac{1}{4} \times 10^{- 5} M . s^{- 1}$

For the reaction; $2 N_{2} O_{5 (g)} \to 4 {NO}_{2 (g)} + O_{2 (g)}$ if the concentration of ${NO}_{2}$ increases by $5.2 \times 10^{- 3} M 100 seconds then the rate of the reaction is$