In the Arrhenius equation for a centrain, the value of A and `E_a` (activation energy ) are `4 xx 10^(13)s^(-1)` and 98.6 kJ `mol^(51)` respectively. If the reaction is of first order, at what termperature will its half-life preriod be 10 min ?

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the given information
We are given:
- Arrhenius factor (A) = \(4 \times 10^{13} \, s^{-1}\)
- Activation energy (\(E_a\)) = 98.6 kJ/mol = \(98.6 \times 10^3 \, J/mol\)
- Half-life (\(t_{1/2}\)) = 10 minutes = 600 seconds
- The reaction is first order.
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