For a first order reaction A → B, the reaction rate at reactant concentration of 0.01 M is found to be 2.0 x 10-5 mol L-1 s-1. The half life period of the reaction is :

To determine the half-life period of the reaction, we need to use the equation for the half-life of a first-order reaction: $t_{1/2}=\frac{0.693}{k}$. We can calculate the rate constant (k) using the equation: $rate=k\times [A]$. So, let's calculate the rate constant: $2.0\times 10^{-5}=k\times 0.01$. Solving for k, we get: $k=\frac{2.0\times 10^{-5}}{0.01}=2.0\times 10^{-3}$. Then, we can calculate the half-life period: $t_{1/2}=\frac{0.693}{2.0\times 10^{-3}}=346.5$. Therefore, the half-life period of the reaction is approximately 347 s.