In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and pure B is 40 mmHg, what is the vapor pressure of component A if the mole fraction of A is 0.6?
Practice Questions
1 question
Q1
In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and pure B is 40 mmHg, what is the vapor pressure of component A if the mole fraction of A is 0.6?
48 mmHg
64 mmHg
80 mmHg
32 mmHg
Using Raoult's Law, the vapor pressure of A in the solution is 0.6 * 80 mmHg = 48 mmHg.
Questions & Step-by-step Solutions
1 item
Q
Q: In a binary solution of A and B, if the vapor pressure of pure A is 80 mmHg and pure B is 40 mmHg, what is the vapor pressure of component A if the mole fraction of A is 0.6?
Solution: Using Raoult's Law, the vapor pressure of A in the solution is 0.6 * 80 mmHg = 48 mmHg.
Steps: 6
Step 1: Understand that we are using Raoult's Law, which states that the vapor pressure of a component in a solution is equal to the mole fraction of that component multiplied by the vapor pressure of the pure component.
Step 2: Identify the given values: the vapor pressure of pure A is 80 mmHg, and the mole fraction of A in the solution is 0.6.
Step 3: Use the formula from Raoult's Law: Vapor Pressure of A in solution = Mole Fraction of A * Vapor Pressure of pure A.
Step 4: Plug in the values: Vapor Pressure of A in solution = 0.6 * 80 mmHg.
Step 5: Calculate the result: 0.6 * 80 = 48 mmHg.
Step 6: Conclude that the vapor pressure of component A in the solution is 48 mmHg.
