The conversion of molecules `X` to `Y` follows second order kinetics. If the concenration of `X` is increased to three times, how will it affect the rate of formation of `Y` ?

Explanation

To solve the problem of how the rate of formation of Y changes when the concentration of X is increased to three times, we can follow these steps:

### Step 1: Understand the Order of the Reaction
The problem states that the conversion of molecules X to Y follows second-order kinetics. This means that the rate of the reaction is proportional to the square of the concentration of X.

### Step 2: Write the Rate Law Expression
For a second-order reaction, the rate law can be expressed as:
\[ \text{Rate} = k [X]^2 \]
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