For a first order reaction, the rate constant (k) is 1.25 X 104 represented as-logk `=14.34-(1.25xx10^4)/T`
Calculate activation energy and Arrhenius factor. At which temperature, the half life of the reaction would be 256 min.

The decomposition of H_(2)O_(2) is a first order reaction . The rate constant of the reaction can be expressed as logk=14.34-(1.25xx10^(4))/(T) . Calculate the activation energy of the reaction . At what temperature does the half-life of the reaction become 265min?

The rate constant for the first order decomposition of H_2O_2 is given by the following by the equation log k= 14.34 - 1.25 xx 10^4 K/T Calculate E-a for this reaction and at what temperature will its half-period be 256 minutes /.

A first order reaction is found to have a rate constant, k= 5.5 xx 10^-14 s^-1 .Find the half-life of the reaction.

Calculate the half-life of a first order reaction from their rate constants: 200s^(-1)

The rate constant of a first order reaction is 2.31xx10^(-3)s^(-1) Calculate the half-life period of the activation energy of the reaction.

The rate constant of a first order reaction follows the equation logk(s^(-1))=22.3-(12.16xx10^(3))/(T)K Find the activation energy of the reaction.

Calculate the half-life of a first order reaction from their rate constants: 4y^(-1)

The rate constant of a first order reaction can be determined by the equation: logk=12.6-(4267)/(T)K. Calculate the energy of activation (E_(a)) and frequency factor (A) of the reaction.

The rate constant of decomposition of B is 4.8xx10^(3)s^(-1) " at "15^(@)C . If the activation energy of the reaction is 80 kJ.mol , at what temperature will the rate constant of the reaction be 1.5xx10^(4)s^(-1) ?

The rate constant for the first order decomposition of H_(2)O_(2) is given by the following equation: logk=14.34-1.25xx10^(4)K//T Calculate E_(a) for this reaction and rate constant k if its half-life period is 256 minutes.