A reaction is of second order with respect to a reactant. How will the rate of reaction be affected if the concentration of this reactant is
reduced to half?

Explanation

To solve the problem, we need to analyze how the rate of a second-order reaction changes when the concentration of the reactant is halved. Let's break it down step by step.

### Step 1: Understand the Rate Law Expression
For a second-order reaction with respect to a reactant A, the rate law can be expressed as:
\[ \text{Rate} = k[A]^2 \]
where \( k \) is the rate constant and \([A]\) is the concentration of the reactant.

### Step 2: Define Initial Concentration
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