What mass of solid that has a molar mass of 46.0 g/mol should be added to 150.0 g of benzene to raise the boiling point of benzene by 6.28°c? (the boiling point elevation constant of benzene is 2.53°c•kg/mol.) use mc029-1.jpg. 2.48 g 8.25 g 17.1 g 43.3 g

Answer : 17.12 g

Explanation:

= elevation in boiling point

= boiling point elevation constant

m= molality

given

Molar mass of solute = 46.0

Weight of the solvent = 150.0 g = 0.15 kg

Putting in the values

x = 17.12 g

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.