Why does a first order reaction never reach completion ?

Show on the basis of rate equation, that a first order reaction does never go to completion.

On the basis of rate equation show that a first order reaction does never go to completion.

The time taken by a first order reaction to reach 10% completion at 298K is the same as the time taken to reach 30% completion at 308K . If value of A=4xx10^(11)s^(-1) , calculate the rate constant at 308K.

In case of first order reaction -

From the rate equation of first order reaction, show first order reaction cannot reach completion.

On the basis of rate equation show that a fist order reaction does never go to completion. For an elementary reaction A + B rarr C , the rate constant increases 10 times on increasing the temperature from 27^@C by 10 degrees, Find out the activation energy of the reaction.

Show that in a first order reaction, time required for completion of 99.9% is 10 times of half-life (t_1/2) of the reaction

Write the equation for the time required for a zero order reaction to reach completion.

How long will it take for a zero order reaction to reach completion if the initial concentration of the reactant is 'a' and its rate constant is 'k' ? What is the half-life of this reaction?

Prove that for any first order reaction time to complete the reaction is infinity but for a zero order reaction, it is a fixed time.