The time taken for 90% of a first order reaction to be completed is approximately

Options

A. 1.1 times that of half-life
B. 2.2 times that of half-life
C. 3.3 times that of half-life
D. 4.4 times that of half-life

Answer

C

Explanation

For a first order reaction,
`k=(2.303)/(t)log.(a)/(a-x)`
`t=(2.303xxt_(1//2))/(0.693)log.(100)/((100-90))[becausek=(0.693)/(t_(1//2))] =3.3t_(1//2)`
=3.3 times that of half-life