For the reaction `2N_(2)O_(5)rarr 4NO_(2)+O_(2)`, if rate 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 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

2N_(2)O_(5)(g)to4NO_(2)+O_(2)(g) What is the ratio of the rate of decomposition of N_(2)O_(5) to rate of formation of NO_(2)

For a reaction, 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) rate of reaction is:

For a reaction, 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) rate of reaction is:

For the reaction : 2N_(2)O_(5) rarr 4NO_(2) +O_(2) , the rate of reaction in terms of O_(2) is d[O_(2)] /dt. In terms of N_(2)O_(5) , it will be :

For the reaction : 2N_(2)O_(5) rarr 4NO_(2) +O_(2) , the rate of reaction in terms of O_(2) is d[O_(2)] /dt. In terms of N_(2)O_(5) , it will be :

In the reaction 2N_2O_(5(g)) rarr 4NO_(2(g)) + O_2 at a certain time. The rate of formation of NO_2 is 0.08 Ms^(-1) . Find the rate of consumption of N_2O_5 , rate of formation of O_2 and the rate of the reaction.

Write the rate law of 2N_(2)O_(5(g))rarr 4NO_(2(g))+O_(2(g)) reaction.