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 get the original -7.6 answer i used the two lowest two points here and subtracted:
x y
3.50E-03 -11.7
3.14E-03 -8.96
3.28E-03 -9.75
(-11.7) - (-8.96)
--------------------------
(3.50x10^-3)-(3.14 x10^-3)
= -7.6111x10^3
To calculate the activation energy (Ea), you first need to determine the slope of the linear graph that represents the relationship between ln(k) (natural logarithm of the rate constant) and 1/T (inverse of temperature).
From the information provided, it seems you have already calculated the slope as -7.6111x10^3.
To convert this slope into activation energy, you need to multiply it by the gas constant (R), which is 8.314 J/(mol·K) or 0.008314 KJ/(mol·K).
So, multiplying the slope (-7.6111x10^3) by the gas constant (0.008314 KJ/(mol·K)) should give you the correct value for the activation energy:
-7.6111x10^3 * 0.008314 = -63.2825 KJ/mol
Therefore, the correct value for the activation energy should be approximately -63.3 KJ/mol.
It seems like someone mentioned multiplying by 2.30. Without knowing the context or the specific formula being used, it's difficult to determine if that factor should be applied or not. It's possible that there might be another step or calculation involved in your particular scenario that requires this additional multiplication. However, based on the information provided, multiplying by 2.30 is not necessary to obtain the activation energy.
If you require further clarification or more details, please provide more information about the specific equation or formula you are using.