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.

one state would change   like louisiana to texas. thats a change

explanation:

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.