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Explain temperature dependency of reaction rate constants and reaction rate from Arrhenius law ?
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written 3.6 years ago by
RakeshBhuse
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• modified 3.6 years ago |
Activation Energy
The minimum amount of energy is requires to start the reaction is known as activation energy.
Arrhenius law
$$\mathrm {k =k_{o}e^{\frac{-E}{RT}}}$$
where,
$\mathrm k=$ rate constant
$\mathrm k_{o} =$ Pre exponential factor
$\mathrm{E} =$ Activation energy, J/mol or cal/mol
$\mathrm R=$ gas constant
$\mathrm T=$ absolute temperature, $\mathrm{K}$ …
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