Chemistry-(general)
NEET Chemistry (general) MCQ Question
Type: MCQ-numerical-Medium-Class 12
Given the vapour pressures of pure acetone and chloroform at 328 K are 741.8 mm Hg and 632.8 mm Hg respectively, calculate the total vapour pressure of an ideal solution with an acetone mole fraction (x_acetone) of 0.4.
A
603.72 mm Hg
B
680.72 mm Hg
C
700.32 mm Hg
D
721.92 mm Hg
Correct Answer
Option B
Detailed Explanation
For an ideal solution, the total vapour pressure is calculated using Raoult's Law: p_total = (x_acetone * p_acetone_pure) + (x_chloroform * p_chloroform_pure). With x_acetone = 0.4, p_acetone_pure = 741.8 mm Hg, and p_chloroform_pure = 632.8 mm Hg, we find p_total = 0.4 * 741.8 + 0.6 * 632.8 = 680.72 mm Hg.
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