Question

The half life of a first order
reaction is 0.5 min. Calculate time
needed for the reactant to reduce to 20% and
the amount decomposed in 55 s.​

Answer 1

Explanation:

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Chemistry

Chemical Kinetics

Integrated Rate Equations

The half life period of a f...

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The half life period of a first order reaction is 20 minutes. The time required for the concentration of the reactant to change from 0.16M to 0.02M is:

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ANSWER

The half life period of a first order reaction is 20 minutes.

t

1/2

=20 minutes.

The rate constant, k=

t

1/2

0.693

=

20min

0.693

=0.03465/min

The time required for the concentration of the reactant to change from 0.16M to 0.02M

is t=

k

2.303

log

a−x

a

=

0.03465/min

2.303

log

0.02

0.16

=60min

Hence, the correct option is B.

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