If `K_(1)=` Rate constant at temperature `T_(1)` and `k_(2)` rate constant at temperature `T_(2)` for a first order reaction, then which of the following relation is correct ?

If k_(1) and k_(2) are rate constants at temperatures T_(1) and T_(2) respectively then according to Arrhenius equation :

If K_1 is the equilibrium constant at temperature T_1 and K_2 is the equilibrium constant at temperature T_2 and If T_2 gt T_1 and reaction is endothermic then

If K_1 is the equilibrium constant at temperature T_1 and K_2 is the equilibrium constant at temperature T_2 and If T_2 gt T_1 and reaction is endothermic then

The activation energies of two reactions are E_(1) & E_(2) with E_(1)gtE_(2) . If temperature of reacting system is increased from T_(1) (rate constant are k_(1) and k_(2) ) to T_(2) (rate constant are k_(1)^(1) and k_(2)^(1) ) predict which of the following alternative is correct.

The activation energies of two reactions are E_(1) & E_(2) with E_(1)gtE_(2) . If temperature of reacting system is increased from T_(1) (rate constant are k_(1) and k_(2) ) to T_(2) (rate constant are k_(1)^(1) and k_(2)^(1) ) predict which of the following alternative is incorrect.

If K _(1) and K_(2) are the rate constants at temperatures T _(1) and T_(2) respectively and E _(a) is the activatino energy, then :

If k_1 and k_2 are rate constants at temperatures T_1 and T_2 respectively, then according to Arrhenius equation,

The activation energies of two reactions are E_(1) and E_(2) (E_(1) gt E_(2)) . If the temperature of the system is increased from T_(1) to T_(2) , the rate constant of the reaction changes from k_(1) to k_(1) in the first reaction and k_(2) to k_(2) in second reaction predict which of the following expression is correct ?

Write the relation between half life t_(1/2) and rate constant (k)of a first order reaction .