A certain substance X has a normal boiling point of 146.3°C and a molal boiling point elevation constant =Kb·1.47°C·kgmol−1. Calculate the boiling point of a solution made of 6.083g of urea NH22CO dissolved in 200.g of X.Round your answer to 4 significant digits.

To solve this problem, we need to use the formula for boiling point elevation, which is ΔTb = Kb * m, where ΔTb is the change in boiling point, Kb is the boiling point elevation constant, and m is the molality of the solution.

Step 1: Calculate the molality of the solution. Molality is defined as the number of moles of solute per kilogram of solvent.

First, we need to find the number of moles of urea. The molar mass of urea (NH2)2CO is approximately 60.06 g/mol.

Number of moles = mass / molar mass = 6.083g / 60.06 g/mol = 0.1012 mol

Then, we convert the mass of the solvent (substance X) from grams to kilograms: 200.0 g = 0.2000 kg

So, the molality (m) = number of moles / mass of solvent in kg = 0.1012 mol / 0.2000 kg = 0.506 mol/kg

Step 2: Use the formula for boiling point elevation to find ΔTb.

ΔTb = Kb * m = 1.47°C·kg/mol * 0.506 mol/kg = 0.7442°C

Step 3: Add ΔTb to the normal boiling point of the substance to find the boiling point of the solution.

Boiling point of solution = normal boiling point + ΔTb = 146.3°C + 0.7442°C = 147.0442°C

Rounding to four significant digits, the boiling point of the solution is 147.0°C.