The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is 0.13 M, it takes ________ min for it to decrease to 0.085 M. The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is 0.13 M, it takes ________ min for it to decrease to 0.085 M. 10. 11 7.0 12 8.0

Respuesta :

Answer:

Therefore it takes 8.0 mins for it to decrease to 0.085 M

Explanation:

First order reaction: The rate of reaction is proportional to the concentration of reactant of power one is called first order reaction.

A→ product

Let the concentration of A = [A]

[tex]\textrm{rate of reaction}=-\frac{d[A]}{dt} =k[A][/tex]

[tex]k=\frac{2.303}{t} log\frac{[A_0]}{[A]}[/tex]

[A₀] = initial concentration

[A]= final concentration

t= time

k= rate constant

Half life: Half life is time to reduce the concentration of reactant of its half.

[tex]t_{\frac{1}{2} }=\frac{0.693}{k}[/tex]

Here [tex]t_{\frac{1}{2} }=0.13 min[/tex]

[tex]k=\frac{0.693}{t_{\frac{1}{2}} }[/tex]

[tex]\Rightarrow k=\frac{0.693}{13 }[/tex]

To find the time takes for it to decrease to 0.085 we use the below equation

[tex]k=\frac{2.303}{t} log\frac{[A_0]}{[A]}[/tex]

[tex]\Rightarrow t=\frac{2.303}{k} log\frac{[A_0]}{[A]}[/tex]

Here ,   [tex]k=\frac{0.693}{13 }[/tex],  [A₀] = 0.13 m and [ A] = 0.085 M

[tex]t=\frac{2.303}{\frac{0.693}{13} } log(\frac{0.13}{0.085})[/tex]

[tex]\Rightarrow t= 7.97\approx 8.0[/tex]

Therefore it takes 8.0 mins for it to decrease to 0.085 M

The time taken is 8 minutes.

The rate of decay of a radioactive substance is given by:

     [tex]-\frac{dN}{dt}=[/tex] λN

here N is the concentraion, λ is the decay constant. If inially the concentration is [tex]N_{0}[/tex]  t time t = 0.

Then solving the above equation we get:

λ = [tex]\frac{2.303}{t}log\frac{N_{0} }{N}[/tex]

Now the half-life is defined as the time after which half of the initial concentration is left. The relation between half-life and decay constant is:

λ = [tex]\frac{0.693}{t_{\frac{1}{2} }}[/tex]  

Given that   [tex]t_{\frac{1}{2} }[/tex] = 13 min

λ = 0.693/13 = 0.0533

So, the time taken for a first-order reaction such that the concentration decreases from 0.13 M to 0.085M can be calculated by following equation:

λ = [tex]\frac{2.303}{t}log\frac{N_{0} }{N}[/tex]

t =  [tex]\frac{2.303}{0.0533}log\frac{0.13 }{0.085}[/tex]

t = 8 min

Learn more about radioactivity:

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