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.

the objects have the same charge is correct.

nathan lee