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)?

1.2596 kJ/mol

Explanation:

Let's consider the Arrhenius equation.

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

its mg hope this

jdjxnbfb

explanation:

jjfnc fdnxnxx