What is the approximate molar mass of a molecular solute if 300 g of the solute in 1000 g of water causes the solution to have a boiling point of 101°c? (kb = 0.512°c/m; kf = 1.86°c/m; molar mass of water = 18 g)

The molar mass of solute is 156 g/mol

Explanation:

Elevation in boiling point is defined as the difference in the boiling point of solution and boiling point of pure solution.

The equation used to calculate elevation in boiling point follows:

= ? °C

Boiling point of pure water = 100°C

Boiling point of solution = 101°C  

Putting values in above equation, we get:

To calculate the elevation in boiling point, we use the equation:

Or,

where,

= 1°C

i = Vant hoff factor = 1 (For non-electrolytes)

= molal boiling point elevation constant = 0.52°C/m.g

= Given mass of solute = 300 g

= Molar mass of solute  = ?

= Mass of solvent (water) = 1000 g

Putting values in above equation, we get:

Hence, the molar mass of solute is 156 g/mol

b.final

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.