The half-life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be [ l o g 2 = 0.301 ]

Step-by-step solution

As k = 0.6932 t 1 / 2 = 0.6932 6.93 m i n - 1 Also t = 2.303 λ l o g [ A o ] [ A ] [ A n ] = initial concentration (amount) [A] = final concentration (amount) So t = 2.303 × 6.93 0.6932 l o g 100 1 = 46.06 m i n u t e s