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Activation energy has a term that is proportional to temperature according to transition state theory (at least).

For instance, for the bimolecular reaction $\ce{A + B -> P}$, we have $E_\mathrm a = \Delta^{\ddagger}H^{\ominus} + nRT$ where $\Delta^{\ddagger}H^{\ominus}$ is standard enthalpy of activation, $n = 2$ for gas reaction and 1 for reaction in solution. This said, for many reactions, the activation enthalpy is much larger than $RT$ (which is ~$\pu{2.5 kJ/mol}$ at $\pu{300 K}$) and the activation energy can be approximately regarded as temperature independent.

Activation energy has a term that is proportional to temperature according to transition state theory (at least). This relies on the definition of activation energy as the parameter

$$E_\mathrm a = RT^2\left(\frac{\mathrm d \ln k}{\mathrm dT}\right)$$

(see this answer).

For instance, for the bimolecular reaction $\ce{A + B -> P}$, we have $$E_\mathrm a = \Delta^{\ddagger}H^{\ominus} + nRT$$ where $\Delta^{\ddagger}H^{\ominus}$ is standard enthalpy of activation, and $n = 2$ for a gas-phase reaction and $1$ for a reaction in solution. That said, for many reactions, the activation enthalpy is much larger than $RT$ (which is ~$\pu{2.5 kJ/mol}$ at $\pu{300 K}$) and the activation energy can be approximately regarded as temperature independent.

Activation energy has a term that is proportional to temperature according to transition state theory (at least). For instance, for the bimolecular reaction $\ce{A + B -> P}$, we have $E_a = \Delta^{\ddagger}H^{\ominus} + nRT$ where $\Delta^{\ddagger}H^{\ominus}$ is standard enthalpy of activation, $n = 2$ for gas reaction and 1 for reaction in solution. This said, for many reactions, the activation enthalpy is much larger than RT (which is ~$\pu{2.5 kJ/mol}$ at $\pu{300 K}$) and the activation energy can be approximately regarded as temperature independent.

Activation energy has a term that is proportional to temperature according to transition state theory (at least). 

For instance, for the bimolecular reaction $\ce{A + B -> P}$, we have $E_\mathrm a = \Delta^{\ddagger}H^{\ominus} + nRT$ where $\Delta^{\ddagger}H^{\ominus}$ is standard enthalpy of activation, $n = 2$ for gas reaction and 1 for reaction in solution. This said, for many reactions, the activation enthalpy is much larger than $RT$ (which is ~$\pu{2.5 kJ/mol}$ at $\pu{300 K}$) and the activation energy can be approximately regarded as temperature independent.

Activation energy has a term that is proportional to temperature according to transition state theory (at least). For instance, for the bimolecular reaction A+ B --> P, we have E$_{a}$=$\Delta^{\ddagger}H^{\ominus}$+nRT where $\Delta^{\ddagger}H^{\ominus}$ is standard enthalpy of activation, n=2 for gas reaction and 1 for reaction in solution. This said, for many reactions, the activation enthalpy is much larger than RT (which is ~2.5 kJ/mol at 300K) and the activation energy can be approximately regarded as temperature independent.

Activation energy has a term that is proportional to temperature according to transition state theory (at least). For instance, for the bimolecular reaction $\ce{A + B -> P}$, we have $E_a = \Delta^{\ddagger}H^{\ominus} + nRT$ where $\Delta^{\ddagger}H^{\ominus}$ is standard enthalpy of activation, $n = 2$ for gas reaction and 1 for reaction in solution. This said, for many reactions, the activation enthalpy is much larger than RT (which is ~$\pu{2.5 kJ/mol}$ at $\pu{300 K}$) and the activation energy can be approximately regarded as temperature independent.