Advertisement Remove all ads

# Solve The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react? - Chemistry

Sum

Solve

The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react?

Advertisement Remove all ads

#### Solution

Given:

Half-life t1/2 = 1.7 hours, [A]= 100%, [A]= 100 - 20 = 80%

To find:

Time for 20% of reactant to react = t

Formulae:

i. t1/2 = 0.693/"k"

ii. "t" = 2.303/"K" "log"_10 ["A"]_0/["A"]_"t"

Calculation:

t1/2 = 0.693/"k"

"k" = 0.693/"t"_"1/2" = 0.693/(1.7 "h") = 0.4076 h-1

t = 2.303/"k" "log"_10 ["A"]_0/["A"]_"t" = 2.303/(0.4076 "h"^-1) "log" 100/80

"t" = 2.303/(0.4076  "h"^-1) xx 0.0969 = 0.5475  "h" xx (60  "min")/(1 "h") = 32.9 min

The time required for 20% of reaction to react is 32.9 min.

Is there an error in this question or solution?
Advertisement Remove all ads

#### APPEARS IN

Balbharati Chemistry 12th Standard HSC for Maharashtra State Board
Chapter 6 Chemical Kinetics
Exercise | Q 4.2 | Page 137
Advertisement Remove all ads
Advertisement Remove all ads
Share
Notifications

View all notifications

Forgot password?