at 17.9 degrees celsus ethyl ether has a vapor pressure of 400 torr. What is the mole fraction of ethly ether in a solution which has a vapor pressure of 380 torr, if the solute is non-volatile at 17.9 degrees celsus?

Pethyl ether = Xethyl ether*P<aup>oethylether

380 = X*400
Solve for X

To find the mole fraction of ethyl ether in the solution, we need to use Raoult's Law, which states that the vapor pressure of a solution is directly proportional to the mole fraction of solvent present.

Let's denote:
P₁ = vapor pressure of pure ethyl ether (400 torr)
P₂ = vapor pressure of the solution (380 torr)
X₁ = mole fraction of ethyl ether in the solution (unknown)

According to Raoult's Law, the vapor pressure of the solution is given by:
P₂ = X₁ * P₁

Rearranging the equation, we can solve for the mole fraction (X₁):
X₁ = P₂ / P₁

Substituting the given values, we have:
X₁ = 380 torr / 400 torr
X₁ ≈ 0.95

Therefore, the mole fraction of ethyl ether in the solution is approximately 0.95.