A solution consisting of 0.228 mol of methylbenzene,C₆H₅CH₃,in 255 g of nitrobenzene,C₆H₅NO₂,freezes at -0.3°C.Pure nitrobenzene freezes at 6.0°C.What is the freezing-point depression constant of nitrobenzene? A) 1.1°C/m B) 27°C/m C) 14.0°C/m D) 3.5°C/m E) 7.0°C/m

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Quizplus · Accepted Answer

The freezing-point depression can be calculated using the formula ΔTf = i * Kf * m, where ΔTf is the change in freezing point, Kf is the freezing-point depression constant, and m is the molality of the solution. The change in freezing point is 6.0°C - (-0.3°C) = 6.3°C. The molality (m) is 0.228 mol / 0.255 kg = 0.894 mol/kg. Solving for Kf gives Kf = ΔTf / m = 6.3°C / 0.894 mol/kg = 7.0°C/m.

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