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Addition of 0.40 g of a compound to 45.5...

Addition of `0.40 g` of a compound to `45.5 m L` of benzene (density `0.879 g mL^(-1)`) lowers the freezing point from `5.51^(@)C` to `4.998^(@)C`.If `K_(f)` for benzene is `5.12 K kg mol^(-1)`,calculate the molar mass of the compound.

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To find the molar mass of the compound, we can follow these steps: ### Step 1: Calculate the change in freezing point (ΔTf) The change in freezing point (ΔTf) is calculated as: \[ \Delta T_f = T_f^{\text{initial}} - T_f^{\text{final}} = 5.51^\circ C - 4.998^\circ C = 0.512^\circ C \] ...
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