Consider the following reaction, the rate expression of which is given below:
\( \text{A} + \text{B} \to \text{C} \)
\(\text{rate} = k [\text{A}]^{1/2} [\text{B}]^{1/2}\)
The reaction is initiated by taking 1M concentration of A and B each. If the rate constant (\(k\)) is \(4.6 \times 10^{-2} \, \text{s}^{-1}\), then the time taken for A to become 0.1 M is ______ sec. (nearest integer)