The Arrhenius equation is
[tex]K=Ae^-{\frac{Ea}{RT}}[/tex]
so if we plot a graph between lnK (natural log of rate constant) and 1/T (inverse of temperature in kelvin)
The straight line equation will be
lnK = lnA - Ea/RT
Where
A = constant for a particular reaction at any temperature
R = gas constant = 8.314 J /molK
So as per this equation the slope of line will be = -Ea/R
Or
Ea = -slope X R
Ea = -(-9.20X10³X 8.314) =76.49kJ /mol
Answer: activation energy = 76.49 kJ /mol
The activation energy for the given reaction is 76.49 kJ/ mo
Activation energy is the minimum amount of energy that is required by the elements to perform any chemical reaction.
[tex]\bold{k = Ae^- \dfrac{-Ea}{RT}}[/tex]
Where,
k = rate constant
A = pre-exponential factor
E_{a} = activation energy (in the same units as R×T)
R = universal gas constant (8.314 J /mol K)
T = absolute temperature (in Kelvin)
[tex]\bold{Ea = -(-9.20\times10^3\times 8.314) =76.49kJ /mol}[/tex]
Thus, the activation energy is 76.49 kJ/ mol.
Learn more about activation energy, here:
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