The decomposition of `H_(2)O_(2)` is a first order reaction. Calculate the half life time and rate constant for the decomposition from the fact that the fraction decomposed in 50 minutes is 0.75

Calculate the half life of the first order reaction from their rate constants given as:

If decomposition of H_(2)O_(2) is a first order reaction , how long would it take to complete one- third of the decomposition ? The rate constant of this decomposition reaction is 3xx10^(-2)"min"^(-1) .

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?

Decomposition of H_(2)O_(2) , is a first order reaction. A 16 volume solution of H_(2)O_(2) of half life 30 min is present at start. When will the solution become one volume?

For a first order reaction the rate constant for decomposition of N_(2)O is 6xx10^(-4)sec^(-1) . The half-life period for the decomposition in seconds is :

The reaction is a first order reaction. The half life period of this reaction is 60 minutes. Calculate the rate constant of this reactions.

The decomposition of sulphuryl chloride to SO_2 and Cl_2 is a first order reaction whose half life is 30 minutes. What percentage of the reactant will be decomposed in 2 hours ?