The rate constants of a reaction at 500 K and 700 K are `0.02 s^(–1) and 0.07 s^(–1)`, respectively. Calculate the values of `E_(a)` and A at 500 K.

Explanation

To solve the problem, we will use the Arrhenius equation, which relates the rate constant (k) of a reaction to the temperature (T) and the activation energy (Ea). The equation is given by:

\[ k = A e^{-\frac{E_a}{RT}} \]

Where:
- \( k \) = rate constant
- \( A \) = pre-exponential factor (Arrhenius constant)
- \( E_a \) = activation energy (in joules per mole)
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