Calculate the molar mass (g/mol) of a nonelectrolyte where 52.80 g of the compound is added to 1.46 kg of solvent. The boiling point of the solution is 102.6ºC and the boiling point of the pure solvent is 99.30ºC. The boiling point elevation constant of the solvent is 2.18 ºC/m
Calculate the molar mass (g/mol) of a nonelectrolyte where 52.80 g of the compound is added to 1.46 kg of solvent. The boiling point of the solution is 102.6ºC and the boiling point of the pure solvent is 99.30ºC. The boiling point elevation constant of the solvent is 2.18 ºC/m
Boiling point is the temperature at which liquid becomes boil ang go to the vapor phase, here the vapor pressure of liquid becomes equal to the surrounding pressure.
When a non volatile solute is added to a particular solvent the the boiling point of the solvent increases. This is called elevation of boiling point. The formula of elevation of boiling point is-
ΔTb =Kb ×m
Here, ΔTb = T _ T0 is the elevation of boiling point where T0 is the boiling point of pure liquid and T is the boiling point of solution.
m is the molality and Kb is the elevation constant.The equation can further be written as,
ΔTb = 1000×Kb×w/ M×W
Where, w= weight of solute
W= weigh of solvent
M= molar mass of solute
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