For the reaction `N_(2)O_(5) rarr 2NO_(2) + (1)/(2) O_(2)`, the rate of disappearance of `N_(2)O_(5)` is `6.25 xx 10^(-3) "mol L"^(-1) s^(-1)`. The rate of formation of `NO_(2)` and `O_(2)` will be respectively.

For the reaction, N_2O_5(g) rarr 2NO_2(g)+1//2O_2(g) , the value of rate of disappearance of N_2O_5 is given as 6.25xx10^(-3) "mol L"^(-1)s^(-1) . The rate of formation of NO_2 and O_2 is given respectively as

In a reaction, the concentration of a reatant (A) changes from 0.200 "mol litre"^(-1) to 0.150 "mol litre"^(-1) in 10 minutes. What is the average rate of reaction during this interval ? N_(2)O_(5)rarr2NO_(2)+_(1//2)O_(2) the rate of disappearance of N_(2)O_(5)"is" 6.5xx10^(-3)"mol" L^(-1)s^(-1) . Computer the rates of formation of NO_(2) and O_(2)

For the reaction 4NH_(3) + 5O_(2) to 4NO + 6H_(2) O , if the rate of disappearance of NH_(3) is 3.6 xx 10^(-3) mol L^(-1) s^(-1) , what is the rate of formation of H_(2) O

For the reaction 2N_(2)O_(5)(g) to 4NO_(2) (g) + O_(2)(g) , the rate of formation of NO_(2)(g) is 2.8 xx 10^(-3) Ms^(-1) . Calculate the rate of disapperance of N_(2)O_(5)(g) .

Decomposition of N_(2)O_(5) is expressed by the equation , N_(2)O_(5)rarr2NO_(2)+^(1//2)O_(2) If during a certain time interval, the rate of decomposition of N_(2)O_(5) is 1.8xx10^(-3) "mol litre"^(-1) "min"^(-1) , what will be the rates of formation of MO_(2) and O_(2) during the same intrval ?

The rate constant for the reaction, 2N_(2)O_(5) rarr 4NO_(2) + O_(2) is 3.0 xx 10^(-5) s^(-1) . If the rate is 2.40 xx 10^(-5) mol L^(-1) s^(-1) , then the initial concentration of N_(2)O_(5) (in mol L^(-1) ) is