Discovering the Molal Boiling-Point-Elevation Constant for CS2

What is the molal boiling-point-elevation constant for CS2?

When 0.260 mol of a nondissociating solute is dissolved in 410.0 mL of CS2, the solution boils at 47.48 oC. Can you determine the molal boiling-point-elevation constant for CS2?

The Molal Boiling-Point-Elevation Constant for CS2

The molal boiling-point-elevation constant for CS2 (Carbon Disulfide) is calculated by using the formula ΔTb = Kb * m, dividing the change in boiling point by the molality of the solute. In this case, the constant is 2.35 °C·kg/mol.

In the realm of Chemistry, the Molal Boiling-Point-Elevation Constant (Kb) is a crucial concept that helps us understand the behavior of solutions. In this specific scenario with CS2, we are tasked with determining the molal boiling-point-elevation constant by analyzing the change in boiling point and the molality of the solute.

The formula ΔTb = Kb * m serves as our guiding principle in this calculation. First, we ascertain the change in boiling point (ΔTb) by subtracting the initial boiling point from the final boiling point, resulting in 1.18 °C.

Next, we calculate the molality (m) by dividing the moles of the solute by the mass of the solvent in kilograms. This gives us a molality of 0.502 mol/kg. Subsequently, by applying the formula ΔTb = Kb * m, we deduce that the molal boiling-point-elevation constant for CS2 is 2.35 °C·kg/mol.

Understanding and utilizing this constant aids in predicting how the boiling point of a solvent will change when a nonvolatile solute is added. It showcases the fascinating interplay between solutes and solvents in solution chemistry.