Consider the following reaction, the rate expression of which is...

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