calculate the boiling point of 25.5g of C7H11NO7S in 1.00x100g H20
To calculate the boiling point of a solution, we need to consider the effect of the solute on the boiling point of the solvent. This can be done using the formula:
ΔTb = Kbm
Where:
ΔTb = change in boiling point (in degrees Celsius)
Kb = boiling point elevation constant for the solvent
m = molality of the solute
To find the boiling point elevation constant (Kb) for water (H2O), we can refer to a reference table or research online. The Kb value for water is approximately 0.512 °C/m.
First, we need to calculate the molality (m) of the solute. The formula for molality is:
m = moles of solute / mass of solvent (in kg)
Given:
- Mass of solute (C7H11NO7S) = 25.5 g
- Mass of solvent (H2O) = 1.00x100 g = 100 g
To find moles of solute, we need to know the molar mass of C7H11NO7S. Let's assume it is 100 g/mol.
Moles of solute = Mass of C7H11NO7S / Molar mass
Moles of solute = 25.5 g / 100 g/mol
Moles of solute = 0.255 mol
Now let's calculate the molality:
m = moles of solute / mass of solvent (in kg)
m = 0.255 mol / 0.100 kg = 2.55 mol/kg
Now we can calculate the change in boiling point (ΔTb):
ΔTb = Kb * m
ΔTb = 0.512 °C/m * 2.55 mol/kg
ΔTb = 1.3068 °C
The boiling point of pure water is 100 °C. Therefore, the boiling point of the solution containing 25.5 g of C7H11NO7S in 1.00x100g H2O would be:
Boiling point of solution = 100 °C + ΔTb
Boiling point of solution = 100 °C + 1.3068 °C
Boiling point of solution ≈ 101.31 °C
Hence, the boiling point of the solution is approximately 101.31 °C.