For the non-equilibrium process, `A + B rarr` Product, the rate is first-order w.r.t. `A` and second order w.r.t. `B`. If `1.0 mol` each of `A` and `B` were inrofuced into `1.0 L` vessel and the initial rate was `1.0 xx 10^(-2) mol L^(-1) s^(-1)`, calculate the rate when half the reactants have been turned into Products.

Explanation

To solve the problem, we need to calculate the rate of the reaction when half of the reactants A and B have been converted into products. Let's go through the steps systematically.

### Step 1: Write the Rate Law Expression
The rate of the reaction is given as first-order with respect to A and second-order with respect to B. Therefore, the rate law can be expressed as:

\[ \text{Rate} = k [A]^1 [B]^2 \]
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