The decomposition of A into product has value of K as `4.5 xx 10^(3) sec^(-1)` at `10^@` C and energy of activation 60 kJ/mol. At what temperature would K be `1.5 xx 10^(4) "sec"^(-1)`.

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:
- \( k \) is the rate constant,
- \( A \) is the pre-exponential factor,
- \( E_a \) is the activation energy,
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