Answer :
Final answer:
The question concerning the boiling point elevation for a benzoic acid solution in methane is incomplete, as the boiling point elevation constant (Kb) for the solvent and the molar mass of benzoic acid are needed to perform the calculation.
Explanation:
Boiling Point Calculation
To calculate the boiling point of a solution containing 0.6 mg of benzoic acid dissolved in 50 g of CH₂ (methane), we need to follow a multistep process involving colligative properties. However, I believe there is an error in the provided information. Normally, for such a calculation, we would need the boiling point elevation constant (Kb) for methane, which is not given, and the molar mass of benzoic acid. The amount of solute and solvent is not sufficient to solve the problem unless the solvent's Kb and the solute's molar mass are known. Boiling point elevation is a colligative property, meaning it is dependent on the number of solute particles in a solution, not the identity of the solute. Benzoic acid's molar mass would be required to convert the mass to moles and calculate molality (mol/kg) for use in the formula: ΔTb = Kb × m, where ΔTb is the boiling point elevation, Kb is the boiling point elevation constant, and m is the molality.
Since there are missing details in the question necessary to perform the calculation, I cannot confidently provide any of the answer choices.
