Respuesta :

Answer:

[tex]Activation\ Energy=2.5\times 10^{-19}\ J[/tex]

Explanation:

As we know that:

[tex]N_v=N\times e^{-\frac {Q_v}{k\times T}[/tex]

Where,

[tex]N_v[/tex] is the number of vacancies

N is the number of defective sites

[tex]{Q_v}[/tex] is the activation energy

k is Boltzmann's constant = [tex]1.38\times 10^{-23}\ J/K[/tex]

T is the temperature

Given temperature = 425°C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (425 + 273.15) K = 698.15 K  

T = 698.15 K

[tex]N_v=2.3\times 10^{13}[/tex]

N = 10 moles

1 mole = [tex]6.023\times 10^{23}[/tex]

So,

N = [tex]10\times 6.023\times 10^{23}=6.023\times 10^{24}[/tex]

Applying the values as:

[tex]2.3\times 10^{13}=6.023\times 10^{24}\times e^{-\frac {Q_v}{1.38\times 10^{-23}\times 698.15}[/tex]

[tex]ln[\frac {2.3}{6.023}\times 10^{-11}]=-\frac {Q_v}{1.38\times 10^{-23}\times 698.15}[/tex]

[tex]Q_v=2.5\times 10^{-19}\ J[/tex]

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