A 7.85 g sample of a compound with an empirical formula C₁H₁ is dissolved in 172 g of benzene. The freezing point of the solution is 1.50$\degree$C below that of pure benzene. Assuming that the compound does not dissociate, what is the molar mass and molecular formula of this compound? The freezing point depression constant for benzene is K_f = 5.12 $\degree$C/m.

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The Answer of A 7.85 g sample of a compound with an empirical formula C₁H₁ is dissolved in 172 g of benzene. The freezing point of the solution is 1.50$\degree$C below that of pure benzene. Assuming that the compound does not dissociate, what is the molar mass and molecular formula of this compound? The freezing point depression constant for benzene is K_f = 5.12 $\degree$C/m.

A 785 G Sample of a Compound with an Empirical Formula