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The rate constant for a reaction is measured as a function of time. A plot is created by graphing ln(k) on the y-axis and 1/T on the x-axis, and a best fit line with a slope of -10,473 K is obtained. Based on this data what is the activation energy of this reaction (in kJ/mol)?

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dsdrajlin

Answer:

1.2596 kJ/mol

Explanation:

Let's consider the Arrhenius equation.

[tex]k=Ae^{-Ea/R.T}[/tex]

where,

k: rate constant

A: pre-exponential factor

Ea: activation energy

R: ideal gas constant

T: absolute temperature

We can take the natural logarithm of the former equation.

ln k = ln A - Ea/R (1/T)

In the plot of ln k vs. 1/T, the slope is -Ea/R. Then,

-10,473 K = -Ea/R

10,473 K = Ea/8.3145 J/mol.K

Ea = 1259.6 J/mol = 1.2596 kJ/mol

The  activation energy of this reaction (in kJ/mol) should be  1.2596 kJ/mol

Calculation of activation energy:

In terms of chemistry, the minimum amount of energy i.e. needed to activate the atoms or molecules with a condition in which they can undergo a chemical transformation.

Here we considered the natural logarithm of the former equation.

ln k = ln A - Ea/R (1/T)

Here

k is  rate constant

A is  pre-exponential factor

Ea is activation energy

R is  ideal gas constant

T is absolute temperature

Now

In the plot of ln k vs. 1/T, the slope is -Ea/R.

So,

-10,473 K = -Ea/R

10,473 K = Ea/8.3145 J/mol.K

Ea = 1259.6 J/mol

learn more about the energy here: https://brainly.com/question/15182235

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