The decomposition of A to B is a first-order reaction with a half-life of 85.9 min when the initial concentration of A is 0.483 M: A → 2B How long will it take for this initial concentration of A to decrease by 23.0%? PLEASE HURRY I DONT HAVE MUCH TIME TO ANSWER THIS
Half life = 85.9 min
Initial concentration of A = 0.483
Use integrated equation of first order.
Ln (At/A0) = - kt
Here At is the concentration at time t.
A0 is the initial concentration.
k is rate constant and t is the time.
Calculate the rate constant using following formula
k = 0.693 / half life = 0.693 / 85.9 min = 0.0080675 min^-1
find out 23 percent of A0
= 0.483 x 23/100
At = 0.483-0.111 = 0.372
Lets plug in all values to get the t
Ln ( 0.372/0.483) = - 0.0080675 x t
t = 32.4 min
so the time required = 32.4 min
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