JEE Main 2024 — 4 April, Shift 2 — Question 79

Consider the following reaction, the rate expression of which is given below $\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$ rate $=\mathrm{k}[\mathrm{A}]^{1 / 2}[\mathrm{~B}]^{1 / 2}$

The reaction is initiated by taking 1 M concentration $A$ and $B$ each. If the rate constant ( k ) is $4.6 \times 10^{-2} \mathrm{~s}^{-1}$, then the time taken for A to become 0.1 M is $\qquad$ sec. (nearest integer)