NEET Chemistry Raoult's Law MCQ Question
A solution is made by mixing 200 g of ethanol (C2H5OH) with 300 g of water. If the vapor pressure of pure water at the same temperature is 24 mmHg and that of pure ethanol is 44 mmHg, calculate the total vapor pressure of the solution, assuming it behaves as an ideal solution.
33.6 mmHg
28.8 mmHg
36.4 mmHg
40.2 mmHg
Correct Answer
Detailed Explanation
Using Raoult's Law, the total vapor pressure is calculated as P_total = x_water * P_water + x_ethanol * P_ethanol, where x is the mole fraction. The solution behaves ideally, so we calculate the mole fractions and apply them to the pure component vapor pressures.
Found an issue with this question?
Related Questions
More from
Calculate the total vapour pressure of an ideal solution at a certain temperature if the mole fraction of component 1 is 0.4, its vapour pressure in p...
Given that the vapour pressures of pure acetone and chloroform at 328 K are 741.8 mm Hg and 632.8 mm Hg respectively, what is the total vapour pressur...
What is the unit of the freezing point depression constant (Kf)?