Respuesta :
Answer : The boiling point of water increases, [tex]2.04^oC[/tex]
Solution : Given,
Moles of solute (sugar) = 4 moles
Mass of solvent (water) = 1 Kg
[tex]K_b=0.51Kg^oC/mole[/tex]
i = 1 for sugar
Formula used :
[tex]\Delta T_b=i\times K_b\times m\\\Delta T_b=i\times K_b\times \frac{n_{solute}}{w_{solvent}}[/tex]
Where,
[tex]\Delta T_b[/tex] = elevation in boiling point
[tex]K_b[/tex] = elevation constant
m = molality
[tex]n_{solute}[/tex] = moles of solute (sugar)
[tex]w_{solvent}[/tex] = mass of solvent (water)
i = van't Hoff factor
Now put all the given values in this formula, we get the elevation in boiling point of water.
[tex]\Delta T_b=(1)\times (0.51Kg^oC/mole)\times \frac{4moles}{1Kg}=2.046^oC[/tex]
Therefore, the elevation in boiling point of water is [tex]2.04^oC[/tex]
