Assuming ideal behavior, determine the mole fraction of acetone in a solution of acetone and water if the vapor pressure of acetone changed from 750mmHg to 735mmHg.

delta P = Xsolute*Poacetone

To determine the mole fraction of acetone in a solution, we need the vapor pressures of both acetone and water at the given condition.

To start, we will use Raoult's Law, which states that the vapor pressure of a component in a solution is directly proportional to the mole fraction of that component.

The equation for Raoult's Law is as follows:

P_total = P_Acetone + P_Water

Where:
P_total is the total vapor pressure of the solution,
P_Acetone is the vapor pressure of acetone, and
P_Water is the vapor pressure of water.

We are given that the initial vapor pressure of acetone (P_Acetone) is 750 mmHg, and the final vapor pressure of acetone (also P_Acetone) is 735 mmHg.

Since we assume ideal behavior, the vapor pressure of water (P_Water) remains constant.

Rearranging the equation, we have:

P_total - P_Water = P_Acetone

Substituting the given values, we get:

P_total - P_Water = 735 mmHg

Now, let's normalize the equation to determine mole fractions.

Divide both sides of the equation by P_total:

(P_total - P_Water) / P_total = 735 mmHg / P_total

The left side of the equation represents the mole fraction of acetone in the solution (let's call it X_Acetone). Thus, we have:

X_Acetone = 735 mmHg / P_total

To find the value of X_Acetone, we need the value of P_total. However, it was not provided in the question. Without this information, we cannot determine the mole fraction of acetone in the solution.