Question

For the reaction: 4 NO2 (g) + O2 (g) 2 N2O5 (g) a) What is the rate of formation of N2O5 in terms of the rate of disappearance of O2? b) If the rate of disappearance of O2 = 0.0037 mol L-1s-1 what is the rate of disappearance of NO2?

Answer 1

`4NO_2+O_2rarr2N_2O_5`

(a)

Since 1 mole of `O_2` is used up for every 2 moles of `N_2O_5` formed the rate of formation of `N_2O_5` will be twice the rate of disappearance of `O_2`.

(b)

Since 4 moles of `NO_2` are used up for every mole of `O_2` the rate of disappearance of `NO_2` will be 4 times the rate of disappearance of `O_2` = `4xx0.0037=0.0148 mol.l^(-1).s^(-1)`