Two different first order reactions have rate consants `k_(1) and k_(2) "at" T_(1)(k_(1)gtk_(2))` . If temperature is increased form `T_(1) "to"T_(2)` ,then new consant become `k_(3) and k_(4)` respeectively. Which among the following relartions is correct

Two different first order reaction have rate constants k_1 and k_2 at T_1(k_1 gt k_2) > If temperature is increased from T_1 " to " T_2 . Then new constants become k_3 and k_4 respectively. Which among the following relations 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 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.

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 ?

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)= 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 :