Calculate the vapor pressure lowering of a solution at 100.0 °c that contains 557.1 g of ethylene glycol (molar mass g/mol). the vapor pressure of pure water at t00.0 °c is 760 torr. (2 points) 62.07 g/mol) in 1000.0 g of water (h20 molar mass 18.02 a) 106 torr b) 0.756 torr c) 760 torr (d)186 torr e) none of these

Answer : E) none of these.

The vapor pressure of solution is 637 torr .

Solution :

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

where,

= vapor pressure of pure solvent  (water) = 760 torr

= vapor pressure of solution  = ?

= mass of solute  (ethylene glycol) = 557.1 g

= mass of solvent  (water) = 1000.0 g

= molar mass of solvent (water) = 18.02 g/mole

= molar mass of solute (ethylene glycol) = 62.07 g/mole

Now put all the given values in this formula ,we get the vapor pressure of the solution.

Therefore, the vapor pressure of solution is, 637 torr.

a physical change biology

explanation: