Question

The conversion of C5H11Br into C5H10 follows first-order kinetics, with a rate constant of 0.385 h-1....

The conversion of C5H11Br into C5H10 follows first-order kinetics, with a rate constant of 0.385 h-1. If the initial concentration of C5H11Br is 0.125 M, find:

(a) the time(hours) at which the concentration will be 3.13 × 10-3 M.

(b) the concentration(M) after 3.2 h of reaction.

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Homework Answers

Answer #1

first order rate constant and concentration related equation is

k = 2.303 / t log[A0/A]

where k = rat econstant given as 0.385h-1

A0 = intial concentration = 0.125 M

A concentration after certain time t

t = time

part A

we havwe to calculate t

A is given as 3.13 × 10-3 M

take the remaining values above and fulg in

0.385 h-1 = 2.303 / t log[0.125 / 3.13 × 10-3 M]

0.385 h-1 = 2.303 / t (1.60)

t = 3.688 / 0.385 h-1

t = 9.6 h

Part B

we have to calulate A

t is given as 3.2 h

0.385 h-1 = 2.303 / 3.2 log[0.125 / A]

log[0.125 / A] = 0.385 h-1 x 3.2 h / 2.303

log[0.125 / A] = 0.535

0.125 / A = 100.535 = 3.43

A = 0.125 / 3.43

A = 0.0364 M

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