# Will increasing the activation energy increase or decrease the rate of a reaction?

From the Arrhenius equation the activation energy (${E}_{a}$) is exponentially inversely proportional to the rate constant ($k$). Because the exponent has a negative sign, increasing the numeric value decreases the resulting exponential term.
$k = A \cdot \text{exp} \left(- \frac{{E}_{a}}{R T}\right)$, $\text{ }$where ${e}^{x} \equiv \text{exp} \left(x\right)$