The vapor pressure of pure water at 15 °c is 12.8 mm hg. what is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (ch3ch2oh, molar mass = 46.07 g/mol) and 22.0 g water?

The vapor pressure of water above this mixture is 5.6173 mm Hg.

Explanation:

We need to find the vapour pressure due to water in the solution.

According to Raoult's law ,

The vapour pressure due to any one component alone is the product of it's pure vapour pressure and it's mole fraction in the solution .

i.e ,

where ,

∴

∴

[tex]Y_A=0.43885*12.8\\Y_A=5.6173 mm Hg[tex]

The vapor pressure of water above this mixture is 5.6173 mm Hg.

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.