Show the time required for 90% completion of a first order reaction is twice for 90% completion of that reaction.

The time taken for 10% completion of a first order reaction is 20mins. Then, for 19% completion, the reaction will take

Why does a first order reaction never reach completion ?

For a first order reaction , show that time required for 99% completion is twice the time required for the completion of 90% of reaction.

Show that for any first order reaction, the time required for the completion of 99.9% of the reaction is 10times the half-life of the reaction.

The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the pre-exponential factor for the reaction is 3.56xx10^(9)s^(-1) , calculate it's rate constant at 318k and also the energy of activation.

The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the value of A is 4xx10^(10)s^(-1) Calculate k at 318 and E_(a)

The time required of 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the pre-exponential factor for the reaction is 3.56xx10^9 S^(-1) . Calculate. Its rate constant at 318K and also the energy of activiation. [R=8.314 JK^(-1) mol^(-1) .

Show that the time required to complete 99% of a 1st order reaction is twice than that of time required to complete 90%.

The time for half life of a first order reaction is 1 hr. what is the time taken for 87.5% completion of the reaction?

Show that the time required to complete a part of first order reaction does not depend on the initial concentration of the reactants.