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What is the new boiling point of a solution when 20.0 g of the covalent compound C₂H₅OH (46 g/mole) is dissolved in 250 g of water? The boiling point elevation constant (K_b) of water is 0.5 °C/m.

A. 100.87 °C
B. 100.3 °C
C. 99.1 °C
D. 112 °C
E. 108 °C

Answer :

Final answer:

To find the new boiling point after adding Ethanol (C2H5OH) to water, we calculate the molality of the solution, then use it along with water's boiling point elevation constant (Kb) to find the change in boiling point. Adding this change to the normal boiling point of water gives us the new boiling point, which is 100.87°C.

Explanation:

To find the new boiling point of a solution after a covalent compound like C2H5OH is dissolved in water, we need to first find the molality of the solution. We know that: Molality (m) = moles of solute / kilogram of solvent Here, moles of Ethanol (C2H5OH) = 20.0 g / 46 g/mol = 0.435 mol and the weight of water is 250g or 0.25 kg.Therefore, the molality, m = 0.435 mol/0.25 kg = 1.74 m.Next, we find the change in boiling point ΔTb = Kb * m. The boiling point elevation constant for water (Kb) is 0.5 °C/m.So, ΔTb = 0.5 °C/m * 1.74 m = 0.87°CFinally, you add the change in boiling point to the normal boiling point of water. The normal boiling point of water is 100°C, so the new boiling point is 100°C + 0.87°C = 100.87°C.

Learn more about Boiling Point Elevation

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