The rate constant (k) for a reaction was measured as a function of temperature. A plot of ln k versus 1>T (in K) is linear and has a slope of -1.01 * 104 K. Calculate the activation energy for the reaction.

8.397J/mol is the activation energy for the reaction

Explanation:

The graphical form of Arrhenius equation is:

ln k = -Ea/R*(1/T)+lnA

Where k is activation energy

Ea is activation energy

R is gas constant (8.314J/molK)

T is absolute temperature

And A is the pre-exponential factor.

The slope of the plot is -Ea/R:

-Ea/R = -1.01x10⁴K

-Ea/8.314J/molK = -1.01x10⁴K

Ea = -1.01x10⁴K*8.314J/molK

Ea = 8.397J/mol is the activation energy for the reaction

h let me think

metric time was an attempt to create a standard unit of time based off of 10, but it never took off an is not included in the metric system (si)