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.

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally