contestada

A mixture of 15. 0 g of the anesthetic halothane (c2hbrclf3 197. 4 g/mol) and 22. 6 g of oxygen gas has a total pressure of 862 torr. What are the partial pressures of each gas?.

Respuesta :

The partial pressure of C₂HBrClF₃ and O₂ are 84 torr and 778 torr respectively.

Given,

Mass of C₂HBrClF₃ = 15.0 g

Mass of O₂ = 22.6 g

Molar mass of C₂HBrClF₃ = 197.4 g/mole

Molar mass of O₂ = 32 g/mole

Raoult's Law:

Psolution = ΧsolventP0solvent

Psolution = vapour pressure of the solution

Χsolvent  = mole fraction of the solvent

P0solvent = vapour pressure of the pure solvent

What is Raoult's Law?

According to Raoult's law, a solvent's partial vapour pressure in a solution (or mixture) is equal to or identical to the pure solvent's vapour pressure multiplied by its mole fraction in the solution.

To learn more on partial pressure from the link:

https://brainly.com/question/13893899

#SPJ4

Otras preguntas