Question

If \(P_A^{0}\) and \(P_B^{0}\) are the vapour pressures of pure liquids A and B, what is the total pressure of an ideal solution where the mole fraction of A is \(0.4\)?

• A. \(0.4P_A^{0} + 0.6P_B^{0}\)
• B. \(0.6P_A^{0} + 0.4P_B^{0}\)
• C. \(P_A^{0} + P_B^{0}\)
• D. \(0.5(P_A^{0} + P_B^{0})\)
• E.

Hint:

For ideal solutions, always apply Raoult's law: total vapour pressure equals the sum of mole fraction multiplied by vapour pressure of each pure component. Remember that \(x_A + x_B = 1\).

Answer 1

The Correct Option is A