If the vapor pressure of pure solvent A is 100 mmHg, and the mole fraction of A in the solution is 0.5, what is the vapor pressure of the solution according to Raoult's Law?
Practice Questions
1 question
Q1
If the vapor pressure of pure solvent A is 100 mmHg, and the mole fraction of A in the solution is 0.5, what is the vapor pressure of the solution according to Raoult's Law?
50 mmHg
100 mmHg
150 mmHg
200 mmHg
According to Raoult's Law, P_solution = X_A * P_A^0 = 0.5 * 100 mmHg = 50 mmHg.
Questions & Step-by-step Solutions
1 item
Q
Q: If the vapor pressure of pure solvent A is 100 mmHg, and the mole fraction of A in the solution is 0.5, what is the vapor pressure of the solution according to Raoult's Law?
Solution: According to Raoult's Law, P_solution = X_A * P_A^0 = 0.5 * 100 mmHg = 50 mmHg.
Steps: 6
Step 1: Identify the vapor pressure of pure solvent A, which is given as 100 mmHg.
Step 2: Identify the mole fraction of solvent A in the solution, which is given as 0.5.
Step 3: Recall Raoult's Law, which states that the vapor pressure of the solution (P_solution) is equal to the mole fraction of the solvent (X_A) multiplied by the vapor pressure of the pure solvent (P_A^0).
Step 4: Substitute the values into the formula: P_solution = X_A * P_A^0.
Step 5: Calculate P_solution by multiplying 0.5 (mole fraction) by 100 mmHg (vapor pressure of pure solvent): 0.5 * 100 mmHg = 50 mmHg.
Step 6: Conclude that the vapor pressure of the solution is 50 mmHg.
