to calculate Ea i solved for slope and i got -7.6111x10^3

so i did this for Ea:

7.61x10^3 x 8.314/mole= 63.3 KJ/Mol

but someone told me im missing the number 2.30? that i have to mulitply

(2.30)(8.314)(7.61x10^3)=?

which is right?

To calculate the activation energy (Ea), you need to use the Arrhenius equation:

k = A * exp(-Ea/RT)

Where:
k is the rate constant
A is the pre-exponential factor
Ea is the activation energy
R is the gas constant (8.314 J/(mol·K))
T is the temperature in Kelvin

Based on your calculations, it seems you have determined the slope of the graph of ln(k) vs. 1/T. However, it appears that you might have made an error in the units for the slope you obtained.

If your slope is correctly determined as -7.6111 x 10^3, it should have the units of K. If that's the case, then you will need to multiply this slope by the gas constant, R, to get the correct value for Ea. However, you have used an incorrect value for R. The gas constant, R, is 8.314 J/(mol·K), not 8.314/mole as you have used in your calculation.

The correct calculation would be:

Ea = slope * R

Ea = (-7.6111 x 10^3 K) * (8.314 J/(mol·K))

Make sure to convert the units properly. Since the activation energy is commonly expressed in kilojoules per mole (kJ/mol), you need to convert J to kJ by dividing by 1000:

Ea = (-7.6111 x 10^3 K) * (8.314 J/(mol·K)) / 1000

Ea ≈ -63.3 kJ/mol

From your calculations, it seems you have obtained approximately -63.3 kJ/mol. Therefore, it appears that the second equation (including the factor of 2.30) is incorrect. The correct result is -63.3 kJ/mol.