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(D) The elevation in boiling point is given by the formula: $\Delta T_{b} = K_{b} 	imes m$. Here,$m$ is the molality,which is defined as $m = \frac{W

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$\frac{\Delta T_{b} 	imes M_{2} 	imes W_{1}}{W_{2}}$

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(D) The elevation in boiling point is given by the formula: $\Delta T_{b} = K_{b} 	imes m$. Here,$m$ is the molality,which is defined as $m = \frac{W_{2} 	imes 1000}{M_{2} 	imes W_{1}}$. Substituting this into the equation: $\Delta T_{b} = K_{b} 	imes \frac{W_{2} 	imes 1000}{M_{2} 	imes W_{1}}$. Rearranging for $K_{b}$: $K_{b} = \frac{\Delta T_{b} 	imes M_{2} 	imes W_{1}}{W_{2} 	imes 1000}$. Note: If the molality is defined as moles per kg of solvent,the $1000$ factor is omitted. Given the options provided,option $D$ represents the relationship where $W_{1}$ is in kg.

Which of the following formulas correctly gives the value of the ebullioscopic constant $(K_{b})$?

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