Question

The second-order rate constant for the decomposition of ClO is 7.53×109 M–1s–1 at a particular temperature. Determine the half-life of ClO when its initial concentration is 1.81×10-8 M.

Answer 1

Answer:

Half life is given by

t1/2 = 136.3s

Explanation:

Peaction Half-life:

The Half-life of a reaction is the time it takes for the reactant concentration to drop to half its original concentration.

For a second order reaction

the time it takes is given by

t1/2 = 1/(k×[A]○

Where k = rate constant and

[A]○ = initial concentration

Therefore

k = 7.53×109 M–1s–1 at a

[ClO]○ its initial concentration = 1.81×10-8 M.

t1/2 = 1/(7.53×109 × 1.81×10-8 )

t1/2 = 136.3 s

Answer 2

The Half life of ClO is 136.3 s.

Half-life for second order reaction:

The Half-life of a reaction is the time it takes for the reactant concentration to drop to half its original concentration.

For a second order reaction, it is given by:

$t_{1/2} = 1/(k*[A]_0)$

where

k = rate constant and

[A]₀ = initial concentration

Given:

k = $7.53*10^9$ $M^{-1}s^{-1}$

[ClO]₀ its initial concentration = $1.81*10^{-8} M$

$t_{1/2} = 1/(7.53*10^9 * 1.81*10^{-8} )\\\\t_{1/2} = 136.3 s$

Thus, half life of ClO is $t_{1/2} = 136.3s$.

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