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. Calculate the half life time and rate constant for the decomposition from the fact that the fraction decomposed in 50 minutes is 0.75

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 :

Decomposition of H_(2)O_(5) follows a first order reaction . In fifty minutes , the concentration of H_(2)O_(2) decreases from 0.5 to 0.125 (M) in one such decomposition when the concentration of H_(2)O_(2) reaches 0.05 (M) , the rate of formation of O_(2) will be -