Calculate the increase in boiling point of a solution made by dissolving 40.0 g of glucose,C₆H₁₂O₆,in 250.0 g of water.K_b for water is 0.52°C/m. A)0.12°C B)0.46°C C)0.59°C D)1.7°C E)83.2°C

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To calculate the increase in boiling point, we use the formula ΔT_b = i * K_b * m, where ΔT_b is the boiling point elevation, i is the van't Hoff factor (which is 1 for glucose since it doesn't ionize in solution), K_b is the ebullioscopic constant of the solvent (water, in this case, 0.52°C/m), and m is the molality of the solution.First, calculate the molar mass of glucose (C6H12O6): (12.01*6) + (1.008*12) + (16.00*6) = 180.16 g/mol.Next, find the number of moles of glucose: 40.0 g / 180.16 g/mol = 0.222 moles.Then, calculate the molality (m) of the solution: 0.222 moles / 0.250 kg of water = 0.888 mol/kg.Finally, calculate the increase in boiling point: ΔT_b = 1 * 0.52°C/m * 0.888 m = 0.462°C, which rounds to 0.46°C.

Calculate the Increase in Boiling Point of a Solution Made