A dilute solution contains m mol of solute A in 1 kg of a solvent with molal elevation constant `K_(b)`. The solute dimerises in solution as `2A hArr A_(2)`. Show that equilibrium constant for the dimer formation is
`K =(K_(b)(K_(b)m-DeltaT))/((2DeltaT_(b)-K_(b)m)^(2))` where `DeltaT_(b)` is the elevation of the boiling point for the given solution. Assume molarity = molarity

Explanation

To solve the problem, we need to derive the equilibrium constant for the dimerization of solute A in a dilute solution. The reaction is given as:

\[ 2A \rightleftharpoons A_2 \]

### Step 1: Define Initial Moles
Let the initial number of moles of solute A be \( m \) (in mol) in 1 kg of solvent.

### Step 2: Define Degree of Dimerization
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