The rate of the reaction :   2N₂O₅ $$ \to $$ 4NO₂ + O₂
can be written in three ways.

$${{ - d\left[ {{N_2}{O_5}} \right]} \over {dt}} = k\left[ {{N_2}{O_5}} \right]$$

$${{d\left[ {N{O_2}} \right]} \over {dt}} = k'\left[ {{N_2}{O_5}} \right];\,\,$$ $${{d\left[ {{O_2}} \right]} \over {dt}} = k''\left[ {{N_2}{O_5}} \right]$$

The relationship between k and k' and between k and k'' are

Which one of the following statements for the order of a reaction is incorrect?

The rate of the reaction, 2NO + Cl₂ $$ \to $$ 2NOCl is given by the rate equation rate = k[NO]²[Cl₂]. The value of the rate constant can be increased by

For the reaction N₂O_5(g) $$ \to $$  2NO_2(g) + 1/2O_2(g)
the value of rate of disappearance of N₂O₅ is given as 6.25 $$ \times $$ 10^$$-$$3 mol L^$$-$$1 s^$$-$$1. The rate of formation of NO₂ and O₂ is given respectively as