What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20^oC to 35^oC?
(R = 8.314 J mol^$$-$$1 K^$$-$$1)

In a reaction, A + B $$ \to $$ product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentration of both the reactants (A and B) are doubled, rate law for the reaction can be written as

In a zero-order reaction, for every 10^oC rise of temperature, the rate is doubled. If the temperature is increased from 10^oC to 100^oC, the rate of the reaction will become

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