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Aneli [31]
3 years ago
6

What is the boiling point elevation constant, Kb, of diethyl ether if 38.2 g of the nonelectrolyte benzophenone, C6H5COC6H5, dis

solved in 330. g of diethyl ether produces a solution that boils at 35.7°C? Use molar masses with at least as many significant figures as the data given.
Chemistry
1 answer:
kakasveta [241]3 years ago
3 0

Answer: the boiling point elevation constant is 1.73^0C/m

Explanation:

Elevation in boiling point is given by:

\Delta T_b=i\times K_b\times m

\Delta T_b=T_b-T_b^0= = Elevation in boling point

i= vant hoff factor = 1 (for non electrolyte)

K_b =boiling point constant = ?

m= molality

\Delta T_b=i\times K_b\times \frac{\text{mass of solute}}{\text{molar mass of solute}\times \text{weight of solvent in kg}}

Weight of solvent (diethylether)= 330 g = 0.33 kg

Molar mass of solute (benzophenone)= 182 g/mol

Mass of solute (benzophenone) = 38.2 g

(35.7-34.6)^0C=1\times K_b\times \frac{38.2g}{182g/mol\times 0.33kg}

K_b=1.73^0C/m

Thus the boiling point elevation constant is 1.73^0C/m

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