Q56. 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 M concentration of 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 $\_\_\_\_$ sec. (nearest integer)
Q56. 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 M concentration of 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 $\_\_\_\_$ sec. (nearest integer)