Question

A particular reactant decomposes with a half-life of 189 s when
its initial concentration is 0.257 M. The same reactant decomposes
with a half-life of 189 s when its initial concentration is 0.753
M.

A) Determine the reaction order.

B) Calculate the rate constant.

Answer #1

A) Determine the reaction order.

The order of reaction is zero because it only depends on the
decomposition of reactive particularly different types of
concentration so that is not a function of a catalyst.

The representation of [A] versus t gives a straight slope - k
ordered in the

origin 0 [A].

These reactions occur in the case of heterogeneous reactions in
which

reaction rate is independent of the concentration of reactants.

B) Calculate the rate constant.

t 1/2= [A]_{0}/2K

k= [A]_{0}/2t 1/2

k=[0.257]_{0}/ 2* 189 s

k=6.79*10^{-4} M/s

...

k=[0.753]_{0}/ 2* 189 s

k=1.99*10^{-3} M/s

A particular reactant decomposes with a half-life of 157 s when
its initial concentration is 0.372 M. The same reactant decomposes
with a half-life of 231 s when its initial concentration is 0.253
M. A.) Determine the reaction order. B)What is the value and unit
of the rate constant for this reaction?

A particular reactant decomposes with a half-life of 169 s when
its initial concentration is 0.293 M. The same reactant decomposes
with a half-life of 245 s when its initial concentration is 0.202
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reaction?

Half-life equation for first-order reactions:
t1/2=0.693k
where t1/2 is the half-life in seconds (s), and
kis the rate constant in inverse seconds (s−1).
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drop to half of its initial value? Express your answer with the appropriate
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c) A...

For a particular first-order reaction, it takes 48 minutes for
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A. 4.8 × 10-4 s-1
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C. 1.0 × 10-4 s-1
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The integrated rate law allows chemists to predict the reactant
concentration after a certain amount of time, or the time it would
take for a certain concentration to be reached. The integrated rate
law for a first-order reaction is: [A]=[A]0e−kt Now say we are
particularly interested in the time it would take for the
concentration to become one-half of its inital value. Then we could
substitute [A]02 for [A] and rearrange the equation to: t1/2=0.693k
This equation caculates the time...

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concentration after a certain amount of time, or the time it would
take for a certain concentration to be reached. The integrated rate
law for a first-order reaction is: [A]=[A]0e−kt Now say we are
particularly interested in the time it would take for the
concentration to become one-half of its initial value. Then we
could substitute [A]02 for [A] and rearrange the equation to:
t1/2=0.693k This equation calculates the time...

a. what order of reaction has a half life that is independent of
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concentration. It is expressed as t1/2=0.693k For a second-order
reaction, the half-life depends on the rate constant and the
concentration of the reactant and so is expressed as
t1/2=1k[A]0
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For a first-order reaction, the half-life is constant. It
depends only on the rate constant k and not on
the reactant concentration. It is expressed as
t1/2=0.693k
For a second-order reaction, the half-life depends on the rate
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t1/2=1k[A]0
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